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LAST MINUTE PACKAGE CHEMISTRY

icse-x Date 16/03/2015

FORGET ABOUT PHYSICS EXAM 2 to 4 pm Take Rest 4 to 5.30 pm Revise ORGANIC CHEMISTRY from Notes and Book 5.30to 6.15 pmSolve following questions 1. An organic compound undergoes addition reactions and gives a red colour precipitate with

ammonical cuprous chloride. Therefore, the organic compound could be: A] Ethane B] Ethene C] Ethyne D] Ethanol 2. The organic compound mixed with ethanol to make it spurious is : A] Methanol B] Methanoic acid C] Methanal D] Ethanoic acid 3. Compound A is bubbled through bromine dissolved in carbon tetrachloride and the product is

CH2Br - CH2Br. (i) Draw the structural formula of A. (ii) What type of reaction has A undergone? (iii) What is your observation? (iv) Name (not formula) the compound formed when steam reacts with A in the presence of

phosphoric acid. (v) What is the producure for converting the product of (b) (iv) back to A? 4. A gaseous hydrocarbon commonly used for welding purposes.Give reason 5. Give reason almost 90% of all known compounds are organic in nature. 6. Give reason it is dangerous to burn methane in an insufficient supply of air. 7. The functional group present in acetic acid is : (A) Ketoneic C + O (B) Hydroxyl –OH (C) Aldehydic –CHO (D) Carboxyl –COOH 8. The unstaturated hydrocarbons undergo : (A) asulbstitution reaction (B) an oxidation reaction (C) an addition reaction (D) none of the above. 9. The number of C–H bonds in ethane molecule are : (A) Four (B) Six (C) Eight (D) Ten 10. Write balanced chemical equations for the following : (i) Monochloro ethane is hydrolysed with aqueous KOH. (ii) A mixture of sodalime and sodium acetate is heated. (iii) Ethanol under high pressure and low temperature is treated with acidified potassium dichromate. (iv) Water is added to calcium carbide. (v) Ethanol reacts with sodium at room temperature. 11. Sodium propionate is treated with dilute hydrochloric acid.Give reaction 12. A reaction in which hydrogen of an alkane is replaced by a halogen. 13. Ethene gas and ethane gas.Differentiate. 14. Identify the statement that is incorrect about alkanes :

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(A) They are hydrocarbons. (B) There is a single covalent bond between carbon and hydrogen (C) They can undergo both substitution as well as addition reactions. (D) On complete combustion they produce carbon dioxide and water. 15. Give balanced equations for the laboratory preparations of the following organic compounds : (i) A saturated hydrocarbon from iodomethane. (ii) An unsaturated hydrocarbon from an alcohol. (iii) An unsaturated hydrocarbon from calcium carbide. (iv) An alcohol from ethyl bromide. 16. Give the structural formulae for the following : (i) An isomer of n-butane. (ii) 2-propanol (iii) Diethyl ether. 17. Give reasons for the following : (i) Methane does not undergo addition reactions, but ethene does. (ii) Ethyne is more reactive than ethane. (iii) Hydrocarbons are excellent fuels. 18. An acid which is present in vinegar. 19. The I.U.P.A.C. name of acetylene is : (a) propane (b) propyne (c) ethene (d) ethyne. 20. The compound formed when ethanol reacts with sodium is ____________ (sodium ethanoate, sodium

ethoxide, sodium propanoate) 21. Hydrocarbons containing a functional group. 22. Preparation of ethane from sodium propionate. 23. Ethane and ethene (using alkaline potassium permanganate solution) (i) Catalytic hydrogenation of ethyne. (ii) Preparation of ethyne from ethylene dibromide. (ii) Preparation of ethanol from monochloroethane and eq. sodium hydroxide. 24. Give the structural formula of the following : (i) ethanol. (ii) l-propanal (iii) ethanoic acid (iv) 1, 2, dichloethane. 1. 200cm3 of acetylene is formed from a certain mass of calcium carbide. Find the volume of

oxygen required and carbon dioxid formed during its complete combustion. The combustion reaction can be represented as :

2. LPG stands for liquefied petroleum gas. Varieties of LPG are marketed including a mixture of propane (60%) and butane (40%). If 10 litre of this mixture is burnt, find the total volume of carbon dioxide gas added to the atmosphere. Combustioin reaction can be represented as :

C3H8(g) + 5 O2(g) 3CO2(g) + 4H2O(g) 2 C4H10(g) + 13O2(g) 8CO2(g) + 10H2O(g)

6.15 to 6.45 pm Rest and have snacks 6.45 to 8.00 pm Revise Lussac’s law, Avogadro’s law, Mole concept, Percentage Composition, EF and MF, Chemical Equation based problems 8 to 9.30 pm Solve following question

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3. State Gau-Lussac's Law of combining volumes.

4. 67.2 l of hydrogen combines with 44.8 litre of nitrogen to form ammonia under specific conditions as :

Calculate the volume of ammonia produced. What is the other substance, if any, that remains in

the resultant mixture. 5. What volume of oxygen is required to burn completely 90 dm3 of butane under similar conditions of

temperature and pressure ? 6 The radio of the mass of a certain volume of gas to the mass of an equal volume of hydrogen under the

same conditions of temperature and pressure. 7. A compound made up two elements X and Y has an empirical formula X2 Y. If the atomic weight

of X is 10 and that of Y is 5 and the compound has a vapour density 25, find its molecular formula. 8. Define the term - Mole. A gas cylinder contains 24 x 1024 molecules of nitrogen gas. If Avogadro’s number is

6 x 1023 and the relative atomic mass of nitrogen is 14, calculate : (i) Mass of nitrogen gas in the cylinder. (ii) Volume of nitrogen at STP in dm3 [ 1120g., 896 dm3] 9. Gas ‘X’ occupies a volume of 100 cm3 at S.T.P. and weighs 0.5g. find its relative molecular mass. 10. Calculate the mass of : (i) 1022 atoms of sulphur. (ii) 0.1 mole of carbon dioxide. [Atomic mass = S = 32, C = 12 and O = 16 and Avogadro's Number = 6 × 1023] 11. The mass of 5.6 dm3 of a certain gas at STP is 12.0. Calculate the relative molecular mass of the gas. 12. The vapour density of a gas is 8. What would be the volume occupied by 24.0 g of the gas at STP? 13. A vessel contains X number of molecules of hydrogen gas at a certain temperature and pressure. How

many molecules of nitrogen gas would be present in the same vessel under the samd conditions of temperature and pressure ?

14. Oxygen oxides ethyne to carbon dioxide and water as shown by the equatiion : 2C2H2 + 5O2 ® 4CO2 + 2H2O What volume of ethyne gas at s.t.p. is required to produce 8.4 dm3 of carbon dioxide at s.t.p.? [H = 1, C =

12, O = 16] 15. (i) Sate Avogadro’s Law. (ii) A cylinder contains 68g of ammonia gas at s.t.p. (1) What is the volume occupied bythis gas? (2) How many moles of ammonia are present in the cylinder? (3) How many molecules of ammonia are present in the cylinder?

[N–14, H–1]

16. The mass of an atom of lead [Pb = 202] Ans.: 33.53 x 10–23 g. 17. The gram - atoms in 88.75g. ofchloine [Cl = 35.5] Ans.: 2.5g

18. The no. of hydrogen atoms in 0.25 mole of H2SO

4. Ans.: 0.5 x 6.023 x 1023 particles

19. The gram molecules in 21g. of nitrogen [ N = 14] Ans.: 0.75 g. molecules 20. The number of atoms in 60g. of neon [ Ne = 20] Ans.: 3 x 6.023 x 1023 atoms 21. The number of moles of ‘X’ atoms in 93g. of ‘X’ [X is phosphorus = 31] Ans.: 3 moles. 22. The moles of sodium hydroxide contained in 160 g of it. [ Na = 23, O = 16, H = 1]Ans.: 4 moles

23. Calculate the percentage by weight of : a] C in carbon dioxide, b] Na in sodium carbonate, c] Al in aluminium nitride. [ C=12, 0=16, H=1, Na=23, A1=27, N=14 ] Ans.: 27.3%, 43.4%, 65.85%

24. Calculate the percentage of iron in K3Fe(CN)6. [ K=39, Fe=56, C=12, N=14] Ans.: 17.02%

N g H g NH g2 2 33 2b g b g b g

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25. Calculate which of the following - calcium nitrate or ammonium sulphate has a higher % of nitrogen. [Ca = 40, 0 = 16, S= 32, N =14] Ans.: 21.21% 17.07%

26. Calculate the percentage of pure aluminium in 10 kg. of aluminium oxide [Al2O3] of 90% purity. [Al = 27, 0 = 16] Ans.: 47.64%

27. State which of the following are better fertilizers- i] Potassium phosphate [K3PO4] or potassium nitrate [KNO3] ii] Urea [NH2CONH2] or ammonium phosphate [(NH4)3PO4] [K= 39, P = 31, 0 = 16, N =14, H =1]

28. Calculate the percentage of carbon in a 55% pure sample of calcium carbonate. [Ca = 40, C = 12, 0 =16] Ans.: 6.6%

29. Calculate the percentage of water of crystallisation in hydrated copper sulphate [CuSO4.5H2O]. [Cu= 63.5, S = 32, 0 = 16, H = 1] Ans.: 36.07%

30. A hydrocarbon contains 82.8% of carbon. Find its molecular formula if its vapour density is 29.[H = 1, C =12] Ans.: C

4H

10

31. An organic compound on analysis gave H = 6.48% and 0 = 51.42%. Determine its empirical formula if the compound contains 12 atoms of carbon. [C = 12, H = 1, 0 = 16] Ans.: C

12H

24O

12

32. A hydrated salt contains Cu = 25.50%, S = 12.90%, 0 = 25.60% and the remaining % is water of crystallization. Calculate the empirical formula of the salt. [Cu = 64, S = 32, 0 = 16, H = 1]

Ans.: CuSO4.5H

2O

34. A gaseous hydrocarbon weighs 0.70 g. and contains 0.60 g. of carbon. Find the molecular formula of the compound if its molecular weight is 70. [C=12, H=1] Ans.: C

5H

10

35. Sample of impure magnesium is reacted with dilute sulphuric acid to give the respective salt and hydrogen. If 1g. of the impure sample gave 298.6 cc. of hydrogen at s.t.p. Calculate the % purity of the sample. [Mg = 24, H = 1] Ans.: 31.99%

36. Calculate the weight of potassium nitrite formed by thermal decomposition of 15.15g of potassium nitrate. [ K = 39, N = 14, O= 16] Ans.: 12.75 gm

37. Copper on reacting with conc. H2SO4 produces copper sulphate. If 1.28 gm of copper is to be converted to copper sulphate. Find i) the weight of the copper sulphate formed and ii) the weight of the acid required. [Cu=64, S=32, O=16] Ans.: 3.2, 3.92

38. From the equation CaCO3 + 2HCl CaCl2 + H2O + CO2. Calculate the weight of CaCl2 obtained from 10g.of CaCO3 and the volume at s.t.p. of CO2 obtained at a same time. [Ca=40, C=12, O=16, Cl=35.5] Ans.: 11.1 & 3.24

39. Combustion of butane takes place as follows : 2C4H10 + 13O28CO2 + 10H2O. Calculate a) the number of moles of oxygen needed for complete combustion of 58g of butane, b) the volume of carbon dioxide formed at s.t.p. at the same time [H=1, C=12] Ans.: 6.5 M & 89.63l

40. Thermal decomposition of calcium nitrate takes place as follows : 2Ca(NO3)22CaO + 4NO2 +O2. If the relative molecular mass of calcium nitrate is 164. a) Calculate the volume of nitrogen dioxide obtained at s.t.p and b) the weight of calcium oxide obtained when 16.4g of calcium nitrate is heated to constant weight [Ca=40, O= 16, N=14] Ans.: (a) 4.48 l (b) 5.6g

41. 2.12g. of an impure mixture containing anhydrous sodium sulphate is dissolved in water. An excess of barium chloride solution is added when 1.74g. of barium sulphate is obtained as a dry precipitate. Calculate the percentage purity of the impure sample. [Na=23, S= 32, O=16, Ba=137] Ans.: 50%

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1. Consider the section of the periodic table given below

You must see the position of the element in the periodic table, while others [shaded] are shown

with a letter. With reference to the table. [i] Which is the most electronegative [ii] How many valence electrons are present in C [iii] Write the formula of the compound between B and H. [iv] In the compound between F and J, what type of bond will be formed [v] Draw the electron dot structure for the compound formed between C and K. 2. Among Period-2 elements A, B, C, D — the one which has high electron affinity is: A] Lithium B] Carbon C] Fluorine D] Neon 3. Define the following term — Ionization potential. 4. An element has an atomic number 16. State (i) the period to which it belongs. (ii) the number of valence electrons. (iii) whether it is a metal or non-metal. 5. Define the following terms : (i) Ionization potential. (ii) Electron affinity. 6. the oxidising power of elements increases on moving from left to right along a period in the

periodic table. 7. Across a period, the ionization potential _________ (increases, decreases, remains same). 8. Down the group, electron affinity _________ (increases, decreases, remains same) 9. In the periodic talbe alkali metals are placed in the group. ....... (A) 1 (B) 11 (C) 17

(D) 18. 10. Give the number of the group and the period of the element having three shells with three

electrons in valence shell. 11. Choose the correct answer from the options given below : (i) An element in period-3 whose electron affinity is zero. (A) Neon (B) Sulphur (C) Sodium (D) Argon (ii) An alkaline earth metal (A) Potassium (B) Calcium (C) Lead (D) Copper 12. Give reason why ionisation potential increases a cross a period. 13. There are three element E, F, G with atomic number 19, 8 & 17. classify the element as metals

and nonmetal. 14. Among the period 2 elements, the element which has high electron affinity is (A) Lithium (B) Carbon (C) Chlorine (D) Fluorine

Group numbers IA IIA IIIA IVA VA VIA VIIA O1 2 13 14 15 16 17 18Li D O J NeA Mg E Si H KB C F G L

9.30 to 10.00 pm Have dinner 10.00 to 11.00 pm Revise PERIODIC TABLE from NOTES and BOOK 11.00 to 11.30 pm Solve following questions

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15.

. In this table H does not represent hydrogen. – Some elements are given in their own symbol and position in the periodic table. – While others are shown with a letter. With reference to the table answer the following questions : (i) Identify the most electronegative element. (ii) Identify the most reactive element of group 1. (iii) Identify the element from period 3 with least atomic size. (iv) How many valence electrons are present in Q? (v) Which element from group 2 would have the least ionization energy? (vi) Identify the noble gas of the fourth period. (vii) In the compound between A and H what type of bond would be formed and give the

molecular formula for the same. 16. The element which has the highest ionization potential. 1I. The one which is composed of all the three kinds of bond [ionic, covalent and corodinate bond]

is : (A) Sodium chloride (B) Ammonia (C) Carbon tetrachloride (D) Ammonium chloride. 2. Draw the structural formula of carbon tetrachloride & state the type of bond present in it. 3I. Match the column A with columb B.

4. Hydrogen chloride can be termed as a polar covalent compound. 5. In covalent compounds, the bond is formed due to the ________ (sharing/transfer) of electrons. 6. Electrovalent compounds have a _________ (low/high) boiling point. 7. By drawing an electron dot diagram, show the lone pair effect leading to the formation of

ammonium ion from ammonia gas and hydrogen ion. 8. Draw an electron dot diagram, to show the structure of hydronium ion. State the type of bonding

present in it. 9. Give the molecular formula of the compound formed between E and G and state the type of

chemical bond in this compound. (E = 19, G = 17)

Group IA IIA IlIA IVA VA VIA VIlA 0number 1 2 13 14 15 16 17 18

2nd

period Li D 0 J Ne

A Mg E Si H M R T I Q u y

Column B(i) Sodium chloride Increase (ii) Ammonium ion Covalent bond(iii) Electronegativity across the period Ionic bond(iv) Non metallic character down the Coordinate bond(v) Carbon tetrachloride Decreases

Column A

Date : 17/03/2015 11.30 pm to 5.30 am Take sound sleep 5.30 am to 6.30 am Get fresh 6.30 am to 7.00 am Revise CHEMICAL BONDING from notes and book 7.00 am to 7.30 am Solve following Questions

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10. A bond formed by a shared pair of electrons with both electrons coming from the same atom. 11. Among the following compounds identify the compound that has all three bonds (ionic, covalent and coordinate bond). (A) Ammonia (B) Ammonium chloride (C) Sodium hydroxide (D) Calcium chloride 12. Which of the following is not a typical property of an ionic compound? (A) High melting point. (B) Conducts electricity in the molten and in the aqueous solution state. (C) They are insoluble in water. (D) They exist as oppositely charged ions even in the solid state. 13. Compare the compounds carbon tetrachloride and sodium chloride with regard to solubility in

water and electrical conductivity. 1. Select the acid which contains four hydrogen atoms in it. A] Formic acid B] Sulphuric acid C] Nitric acid D] Acetic acid 2. A black coloured solid which on reaction with dilute sulphuric acid forms a blue

coloured solution is A] Carbon B] Manganese [IV] oxide C] Lead [II] oxide D] Copper [II] oxide 3. Solution A is a strong acid, Solution B is a weak acid, Solution C is a strong alkali i] Which solution contains solute molecules in addition to water molecules ii] Which solution will give a gelatinous white precipitate with zinc sulphate solution The precipitate disappears when an excess of the solution is added. iii] Which solution could be a solution of glacial acetic acid iv] Give an example of a solution which is a weak alkali. 4. Write the equation[s] for the reaction[s] to prepare lead sulphate from lead carbonate. 5. Define the following term — Neutralization 6. The diagram given below is to prepare Iron[III] chloride in the laboratory:

i] What is substance B ii] What is the purpose of B iii] Why is iron[III] chloride to be stored in a closed container iv] Write the equation for the reaction between iron and chlorine. 7. An example of a complex salt is : (A) Zinc sulphate

7.30 am to 9 am Revise ACIDS BASES AND SALTS from notes and book 9 to 9.30 am Have breakfast 9.30 to 10 am Take Rest 10 to 11 am Solve following questions

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(B) Sodium hydrogensulphate (C) Iron (II) ammonium sulphate (D) Tetrammine copper (II) sulphate 8. Give the equations for the following conversions A to E.

9. Name the method used for preparation of the following salts from the list given below : (i) Sodium nitrate (ii) Iron (III) chloride (iii) Lead chloride (iv) Zinc sulphate (v) Sodium hydrogen sulphate. List : (A) Simple displacement (B) Neutralization (C) Decomposition by acid (D) Double decomposition (E) Direct synthesis. 10.

11. From the list given below, select the word(s) required to correctly complete blanks (i) to

(v) in the following passage. The words from the list are to be used only once. Write the answers as (a) (i), (ii), (iii) and so on. Do not copy the passage.

[ammonia, ammonium, carbonate, carbon dioxide, hydrogen, hydronium, hydroxide, precipitate, salt, water]:

(i) A solution M turns blue litmus red, so it must contain (i) _____ Ions; another solution O turns red litmus blue and hence, must contain (ii) _____ ions. (ii) When solutions M and O are mixed together, the products will be (iii) _____ and (iv) _____ (iii) If a piece of magnesium was put into a solution M, (v) _____ gas would be evolved.

ZnSO4

AZnCO3

B Zn(NO )3 2

C

Zn(OH)2ZnO

E

Column A Column B1 Acid salt A Ferrous ammonium

sulphate2 Double salt B Contains only ions3 Ammonium

hydroxide solutionC Sodium hydrogen

sulphate4 Dilute hydrochloric

acidD Contains only

molecules5 Carbon tetrachloride E Contains ions and

molecules

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12. A salt formed by incomplete neutralisation of an acid by a base. 13. A definite number of water molecules bound to some salts. 14. The process in which a substance absorbs moisture from the atmospheric air to

become moist, and ultimately dissolves in the absorbed water. 15. Which one of the following will not produce an acid when made to react with water? (A) Carbon monoxide (B) Carbon dioxide (C) Nitrogen dioxide (D) Sulphur trioxide. 16. Identify the metallic oxide which is amphoteric in nature: (A) Calcium oxide (B) Barium oxide (C) Zinc oxide (D) Copper (II) oxide. 17. Choosing the substances from the list given below, write balanced chemical equations

for the reactions which would be used in the laboratory to obtain the following salts: Copper ,, Copper(II) carbonate, Dilute Sulphuric acid,Iron ,

Sodium carbonate Sodium, Sodium chloride,Zinc nitrate (i) Sodium sulphate (ii) Zinc carbonate (iii) Copper(II) sulphate (iv) Iron(II) sulphate.

1. Name the gas evolved [formula is not acceptable].

The gas produced by the action of concentrated sulphuric acid on sodium chloride. 2. Match each substance A to E listed below with the appropriate description given below: [A] Sulphur [B] Silver chloride [C] Hydrogen chloride [D] Copper [II] Sulphate [E] Graphite. [i] A covalent compound which behaves like an ionic compound in aqueous

solution. [ii] A compound which is insoluble in cold water but soluble in excess of ammonia

solution. 3. Write a fully balanced equation for each of the following [i] Red lead is warmed with concentrated hydrochloric acid. [ii] Magnesium metal is treated with dilute hydrochloric acid. 4. Correct the following statement. Hydrochloric acid is prepared in the laboratory by passing hydrogen chloride directly

through

11 to 1.00 pm Revise all compounds from notes and book. 1 pm to 1.30 pm Have lunch 1.30 to 2.30 pm Take Rest 2.30 to 3.30 pm Solve following questions HYDROGEN CHLORIDE

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5. The diagram shows an apparatus for the laboratory preparation of hydrogen chloride. (i) Identify A and B. (ii) Write the equation for the reaction.

(iii) How would you check whether or not the gas jar is filled with hydrogen chloride?

(iv) What does the method of collection tell you about the density of hydrogen chloride?

6. Hydrogen chloride gas being highly soluble in water is dried by : (A) Anhydrous calcium chloride (B) Phosphorous penta oxide (B) Quick lime (D) Concentrated sulphuric acid. 7. Write the balanced chemical equation for each of the following reactions : (i) Sodium thiosulphate is reacted with dilute hydrochloric acid (ii) Calcium bicarbonate reacts with dilute hydrochloric acid 8. In laboratory preparaton of hydrochloric acid, HCl gas is dissolved in water. (i) Draw a diagram to show the arrangement used for the absorption of HCl in water. (ii) Why is such an arrangement necessary? Give two reasons. (iii) Write the chemical equations for the laboratory preparation of HCl gas when the

reactants are : (A) below 200 oC (B) above 200 oC. 9. Aqua regia contains one part by volume of nitric acid and three parts by volume of

hydrochloric acid give reaction for aqua regia mixture. 10. Concentrated hydrochloric acid and potassium permaganate solution is mixed. Give

reaction and observation. 11. Potassium sulphite is treated with dilute hydrochloric acid. 12. Concentrated hydrochloric acid is made to react with manganese 13. Copper sulphide is treated with dilute hydrochloric acid.

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AMMONIA 1. Name the gas evolved in each case [ formula is not acceptable]. The gas that burns in oxygen with a green flame. 2. Write a fully balanced equation for the following : Magnesium nitride is treated with warm water. 3. Identify the substance ‘Q’ based on the information given below : The white crystalline solid ‘Q’ is soluble in water. It liberates a pungent smelling gas

when heated with sodium hydroxide solution. 4. The questions below are related to manufacture of ammonia. (i) Name the process. (ii) In what ratio must the reactants be taken? (iii) Name the catalyst used. (iv) Give the equation for the manufacture of ammonia. (v) Ammonia can act as a reducing agent - write a relevant equatioin for such a

reactioin. 5. Ammonium hydroxide is first adedina small quantity and then in excess to a solution of

copper sulphate. 6. Water is added to the product formed, when aluminium is burnt in a jar of nitrogen gas. 7. The diagram shown an experimental set up for the laboratory preparation of a pungent

smelling gas. The gas is alkaline in nature. (i) Name the gas collected in the jar. (ii) Write the balanced equation for the above preparaton. (iii) How is the gas being collected? (iv) Name the drying agent used. (v) How will you find that the jar is full of gas? 9. The gas produced when excess ammonia reacts with chlorine. 10. Excess ammonia hydroxide solution is added to lead nitrate solution. Give reaction. 11. Ammonia and Oxygen in the presence of a catalyst. 12. Explain why ammonium nitrate is not used in the preparation of ammonia. 13. Excess of chlorine gas is reacted with ammonia gas. 14. A few drops of dilute hydrochloric acid are added to silver nitrate solution. 16. Nitrogen gas can be obtained by heating : (A) Ammonium nitrate. (B) Ammonium nitrite. (C) Magnesium nitride. (D) Ammonium chloride. 17. Reduction of hot Copper(II) oxide to copper using ammonia gas. 18. Oxidation of carbon with concentrated nitric acid. 19. An alkaline gas which produces dense white fumes when reacted with hydrogen

chloride gas. 20. A gas which does not conduct electricity in the liquid state but conducts electricity when

dissolved in water. 21. Ammonia gas is collected by __________ (an upward displacement of air, a downward

displacement of water, a downward displacement of air) 22. Action of warm water on magnesium nitride.

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23. When calcium hydroxide is heated with ammonium chloride crystals. 24. Name the other ion formed when ammonia dissolves in water. 25. Give one test that can be used to detect the presence of the ion produced. 26. Catalytic oxidation of ammonia to nitric oxide.

NITRIC ACID

1. Name the gas evolved [formula is not acceptable]. The gas produced by the action of dilute nitric acid on copper. 2. Match each substance A to E listed below with the appropriate description given below

: A] Sulphur B] Silver chloride C] Hydrogen chloride D] Copper [II] Sulphate E] Graphite A non-metal which reacts with concentrated nitric acid to form its own acid as one of

the product. 3. Correct the following statement. Copper reacts with nitric acid to produce nitrogen dioxide. 4. What is the special feature of the apparatus that is used in the laboratory preparation

of nitric acid? 5. Why should the temperature of the reaction mixture of nitric acid not be allowed to rise

above 200 oC? 6. Ferric hydroxide react with HNO3.

7. The gas produced when copper reacts with concentrated nitric acid. 8. Zinc nitrate crystals are strongly heated. What will you observed. 9. Magnesium react with nitric acid to librate hydrogen gas. Supply missing word. 10. Iron is rendered passive with fuming nitric acid. Give reason. Give balance equation of

dil HNO3 and Cu(NO3)2.

SULPHURIC ACID

1. Sulphur is treated with concentrated nitric acid. 2. A few crystals of KNO3 are heated in a hard glass test tube.

3. Lead nitrate crystals are heated in a hard glass test tube. 4. Oxidation of carbon with concentrated nitric acid. 5. Cold, dilute nitric acid reacts with copper to form ________ (Hydrogen, nitrogen

dioxide, nitric oxide). 6. Action of heat on a mixture of copper and concentrated nitric acid. 7. Laboratory preparation of nitric acid.

8. Sugar crystals are added to a hard glass test tube containing concentrated sulphuric acid.

9. When dilute sulphuric acid reacts with iron sulphide, the gas evolved is _____. (A)Hydrogen sulphide (B) Sulphur dioxide

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(C) Sulphur trioxide (D)Vapour of sulphuric acid. 10. Dilute sulphuric acid is poured over sodium sulphite 11. With the help of equations, give an outline for the manufacture of sulphuric acid by the

contact process. 12. What property of sulphuric acid is shown by the reaction of concentrated sulphuric acid

when heated with (A) potassium nitrate (B) carbon? 13. Properties of H2SO4 are listed below. Choose the property A, B, C or D which is

responsible for the reactions (i) to (v). A: Acid B: Dehydrating agent C: Non-volatile acid D: Oxidizing agent

(i) Cl2H22O11 + nH2SO4 12C + 11H2O + nH2SO4, (ii) S + 2H2SO4 3SO, + 2H2O, (iii) NaCl + H2SO4NaHSO4 + HCl, (iv) CuO + H2SO4CuSO4 + H2O, (v) Na2CO3 + H2SO4 Na2SO4 + H2O + CO2 [Some properties may be repeated] 14. Concentrated sulphuric acid is added drop wise to a crystal of hydrated copper

sulphate. 15. In the given equation identify the role played by concentrated sulphuric acid (A) Non-volatile acid (B) Oxidising agent (C) Dehydrating agent (D) None of above (1.) Dehydration of concentrated sulphuric acid with sugar crystals. (2.) Action of concentrated sulphuric acid on carbon. (3.) Any two condition for the conversion of sulphur dioxide to sulphur trioxide. (4). Give one equation each to show the following properties of sulphuric acid : (i) Dehydrating property. (ii) Acidic nature. (iii ) As a non-volatile acid.

1. Carbon dioxide and sulphur dioxide gas can be distinguished by using : A] moist blue litmus paper B] lime water C] acidified potassium dichromate paper D] none of the above 2. Identify the substance ‘R’ based on the information given below : The pale green solid ‘R’ turns reddish brown on heating. Its aqueous solution gives a white precipitate

with barium chloride solution. The precipitate is insoluble in mineral acids.

3.30 to 4 pm Revise ANALYTICAL AND PRACTICAL CHEMISTRY 4 to 4.30 pm Solve following questions

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3. The action of heat on the blue crystalline solid L gives a reddish brown gas M, a gas which re-lights a glowing splint and leaves a black residue. When gas N, which has a rotten egg smell, is passed through a solution of L a black precipitate is formed. (i) Identify L, M and N (Name or formula) (ii) Write the equation for the action of heat of L (iii) Write the equation for the reaction between the solution of L and the gas N. 4. Lead nitrate solution is added to sodium chloride solution

5. Zinc is heated with sodium hyroxide solution.

6. Sodium hydroxide solution is added to the solutions containing the iron mentioned in List X. List Y gives the detail of the precipitate. Match the ions with their coloured precipitates.

7. Write observation and reaction for following:

1. Sodium chloride solution and sodium nitrate solution. 2. Hydrogen chloride gas and hydrogen sulphide gas. 3. Calcium nitrate solution and zinc nitrate solution. 4. Carbon dioxide gas and sulphur dioxide gas. 5. Ammonium hydroxide solution is added to copper (II) nitrate solution in small quantities and then

in excess. 6. Ammonium hydroxide solution is added to zinc nitrate solution in minimum quantities and then in

excess. 7. A dilute mineral acid which forms a white precipitate when treated with barium chloride solution. 8. Distinguish between the following pairs of compounds using the test given within brackets : (i) Iron (II) sulphate and iron (III) sulphate (using ammonium hydroxide) (ii) A lead salt and a zinc salt (using excess ammonium hydroxide) (iii) Sodium nitrate and sodium sulphite (using diute sulphuric acid) (iv) Dilute sulphuric acid and dilute hydrochloric acid (using barium chloride solution) 9. (i) When dilute hydrochloric acid is added to sodium carbonate crystals. (ii) When excess sodium hydroxide is added to calcium nitrate solution. (iii) When moist starch iodide paper is introduced into chlorine gas. 10. State the inference drawn from the following observations : (i) On arrying out the flame test with a salt P a brick red flame was obtained. What is the cation in P? (ii) A gas Q turns moist lead acetate paper silvery black. Identify the gas Q.

(iii) pH of liquid R is 10. What kind of substance is R? (iv) Salt S is prepared by reaching dilute sulphuric acid with copper oxide. Identify S.

(i) Pb2+ A. Reddish brown

(ii) Fe2+ B. White insoluble in excess

(iii) Zn2+ C. Dirty green

(iv) Fe3+ D. White soluble in excess

(v) Cu2+ E. White soluble in excess

(vi) Ca2+ F. Blue

List X List Y

TIWARI TUTORIALS

1. Mr.Ramu wants to electroplate his key chain with nickel to prevent rusting. For this electroplating:

(i) Name the electrolyte (ii) Name the cathode ‘ (iii) Name the anode (iv) Give the reaction at the cathode (v) Give the reaction at the anode. 2. Three different electrolytic cells A, B and C are connected in separate circuits. Electrolytic cell A

contains sodium chloride solution. When the circuit is completed a bulb in the circuit glows brightly. Electrolytic cell B contains acetic acid solution and in this case the bulb in the circuit glows dimly. The electrolytic cell C contains sugar solution and the bulb does not glow. Give a reason for each of these observations.

3. Differentiate between electrical conductivity of copper sulphate solution and copper metal. 4. During the electrolysis of copper (II) sulphate solution using platinum as cathode and carbon as anode : (i) What do you observe at the cathode and at the anode?

(ii) What change is noticed in the electrolyte? (iii) Write the reactions at the cathode and at the anode. 5. Cations migrate during electrolysis supply missing words. 6. Select the correct answer from the list given in brackets: (i) An aqueous electrolyte consists of the ions mentioned in the list, the ion which could be

discharged most readily during electrolysis. [Fe2+, Cu2+, Pb2+, H+] (ii) The metallic electrode which does not take part in an electrolytic reaction. [Cu, Ag, Pt, Ni]. (iii) The ion which is discharged at the anode during the electrolysis of copper sulphate solution

using copper electrodes as anode and cathode. [Cu2+, OH–, SO42–, H+]

(iv) When dilute sodium chloride is electrolysed using graphite electrodes, the cation is discharged at the cathode most readily. [ Na+, OH–, H+, Cl–1].

7. Electricity is passed through molten lead bromide.Give observation. 8. Which of these will act as a non-electrolyte ? (A) Liquid carbon tetrachloride (B) Acetic acid (C) Sodium hydroxide aqueous solution acid. (D) Potassium chloride aqueous solution. 8. Copper sulphate solution is electrolysed using copper electrodes. Study the diagram given below and answer the question that follows :

4.30 to 5.30 pm Revise ELECTROLYSIS from notes and book 5.30 to 6.30 pm Solve following questions

TIWARI TUTORIALS

(i) Which electrode to your left or right is known as the oxidising electrode and why ? (ii) Write the equation representing the reaction that occurs. (iii) State two appropriate observation for the above electrolysis reaction. 9. When fused lead bromide is electrolysed we observe : (a) a silver grey deposit at anode and a reddish brow deposit at cathode (b) a silver grey deposit at cathode and a reddish brown deposit at anode (c) a silver grey deposit at cathode and reddish brown fumes at anode (d) silver grey fumes at anode and reddish brown fumes at cathode. 10. The electrolyte used for electroplating an article with silver is : (a) silver nitrate solution (b) silver cyanide solutioin (c) sodiumargentocyanide (d) nickel sulphate solution. 11. At the cathode when acidified aqueous copper sulphate solution is electrolyzed with copper electrodes. 12. Name the kind of particles present in : (i) Sodium Hydroxide solution. (ii) Carbonic acid. (iii) Sugar solution.

1. The substance is an alloy of zinc, coper and tin.

2. Answer the following questions : (i) Name a metal which is found abundantly in the earth's crust. (ii) What is the difference between calcination and roasting? (iii) Name the process used for the enrichment of sulphide ore. (iv) Write the chemical formulae of one main ore of ironand aluminium. (v) Write the constituents of electrolyte for the extraction of aluminium.

4. The metals zinc and tin are present in the alloy. (A) Solder (B) Brass (C) Bronze (D) Duralumin.

List 1 List 21 The alloy contains Cu and Zn, is hard silvery and is

used in decorative articlesA Duralumin

2 It is stronger than Aluminium, light and is used in making light tools.

B Brass

3 It is lustrous, hard, corrosion resistant and used in surgical instruments.

C Bronze

4 Tin lowers the melting point of the alloy and is used for soldering purpose.

D Stainless steel

5 The alloy is hard, brittle, takes up polish and is used for making status

E Solder

6.30 to 7.30 pm Revise METALLURGY from notes and book 7.30 to 8.00 pm Solve following questions

TIWARI TUTORIALS

5.

Using the information above, complete the following: (i) _____ is the metallic element. (ii) Metal atoms tend to have a maximum of _____ electrons in the outermost energy level. (iii) None-metallic elements tend to form _____ oxides while metals tend to form _____ oxides. (iv) Non-metallic elements tend to be _____ conductors of heat and electricity. (v) Metals tend to _____ electrons and act as _____ agents in their reactions with elements and

compounds. 6. The following questions relate to the extraction of aluminium by electrolysis : (i) Name the other aluminium containing compound added to alumina and state its

significance. (ii) Give the equation for the reaction tha takes place at the cathode. (iii) Explain why is it necessary to renew the anode periodically 7. The main ore used for the extraction of iron is : (a) Haematite (b) Calamine (c) Bauxite (d) Cryolite 8. Heating an ore in a limited supply for air or in the basence of air at a temperature just below its

melting point is known as : (a) smelting (b) ore dressing (c) calcination (d) bessemerisation 9. Sluminium powder used in thermite welding because : (a) it is a strong reducing agent (b) it is a strong oxidising agent (c) it is corrosion resistant (d) it is a good conductor of heat. 10. State the main components of the following alloys : (i) Brass. (ii) Duralumin. (iii) Bronze. 11. Name the following : (i) The property possessed by metals by which they can be beaten into sheets. (ii) A compound added to lower the fusion temperature of electrolytic bath in the extraction of

aluminium. (iii) The ore of zinc containing its sulphide.

X Y

Normal Electric Configuration 2, 8, 7 2, 8, 2

Nature of oxideDissolves in water and turns blue

litmus redVery low solubility in water. Dissolves

in hydrochloric acid

Tendency for oxidis ing and reducing reactions

Tends to oxidise elements and compounds

Tends to act as a reducing agent

Electrical and thermal conductivity

Very poor electrical conductor Poor thermal conductivity

Good Electrical conductor Good Thermal conductor

Tendency to form alloys and amalgums No tendency to form alloys Forms alloys

TIWARI TUTORIALS

SECTION - A Q1. Name one substance in each case, to which the following descriptions could apply. (a) (i) The alkali added to an ammonium salt to obtain ammonia in the laboratory. (ii) The oxidised product obtained when concentrated nitric acid reacts with-a metal, which on thermal

decomposition leaves a black residue and evolves a reddish brown gas. (iii) The substance which on thermal decomposition gives a metallic oxide which on electrolytic

reduction gives a trivalent metal. (iv) A salt formed when a yellow non-metallic element reacts with a metal below zinc. in the activity

series. (v) A basic oxide which dissolves in water to give a monoacidic base. [5] (b) Answer the following pertaining to the tests used for identifying gases and acids. (i) Hydrochloric acid reacts with silver nitrate solution to give a white precipitate .State the solubility

of the precipitate in liquor ammonia. (ii) Name the complex salt whose solution turns pale brown on passage of ammonia through it.’ (iii) Copper reacts with both concentrated nitric acid and concentrated sulphuric acid on heating

liberating two different acidic gases. Give balanced equations for the two reactions. (iv) Give a chemical test to distinguish the gases obtained in (b) (v) Give a chemical test to distinguish dilute nitric acid and dilute sulphuric acid using a salt solution

only. . [5] (c) (i) State Avogadro’s law. (ii) If ‘x’ molecules of hydrogen combine with ‘x’ molecules of chlorine, how many molecules will the

product formed contain. (iii) Fill in the blanks with the correct answer: 1. The mass of oxygen which will combine with8 g. of hydrogen to form water is ....................... 2. The number of molecules in 1.5 kg. of lead chloride is ........................ [Pb = 207, Cl = 35.5] 3. 0.1 moles of oxygen contains —”- atoms. [10] 4. The gram molecules in 192 g. of sulphur dioxide is ................................ [S = 32, 0 = 16] 5. 300 ml. of ethane undergoes complete combustion with 1500 cc, of oxygen. The volume of

unused oxygen is ....... (d) Complete the electrode reactions given below by filling in the blanks with the correct symbols or ions. [5] (i) Electrolysis of aqueous copper sulphate using copper electrodes. At anode : Cu – 2e– ______ (ii) Electrolysis of acidified water using platinum electrodes. At anode : 4OH l– – ____ 4OH 4 OH ____ + _____ (iii) Dissociation of sodium silver cyanide solution. Na[Ag(CN)2] — + — + —’ (iv) Dissociation of pure alumina. Al2O3 ______ + ______ Reaction at cathode: 2A13 + — 2Al. (v) Electrolysis of fused lead bromide using inert electrodes. PbBr2 —— + —— Reaction at cathode :Pb2+ + _____ ______

8 to 9.30 pm Solve following

FULL LENGTH paper TEST PAPER

Section I is compulsory and attempt any four questions from Section II. The intended marks for questions or parts of questions, are given in bracket [ ]

TIWARI TUTORIALS

(e) Answer the following as per the instruction in bracket. (i) Li, C, O, S, F, Ne [State the element’ not present in Period-2 of the Periodic Table]. (ii) Cl, P, Al; S, Mg, Na [Arrange the elements in increasing order of electronegativity] (iii) Br2, HF, HCI, H2O, HI [State the liquid which is a non-polar covalent compound]. (iv) O2, Cl2, F2, NH3, N2, H2 [State the gas which is a reducing agent]. (v) Aluminium, calcium, zinc, silver, nickel [State the metal which shows variable valency]. . (vi) Carbonic acid, lactic acid, dilute sulphuric acid, ammonium hydroxide, sodium hydroxide [Arrange

the substances in decreasing order of pH values]. (vii) Lead [II] chloride, lead carbonate, silver chloride, ammonium chloride. [State the salt not prepared

by precipitation - double decomposition). (viii) Fe (OH)2, Cu(OH)2, Pb(OH)2, Fe(OH)3, Zn(OH)2 [State the hydroxide soluble in excess of

sodium hydroxide solution]. (f) Narne and state the following laws: (i) The law which relates to the number of molecules in specific volumes of gases. (ii) The law which correlates periodicity of properties of elements with their atomic numbers. [2] (g) Give balanced equations for the following reactions. [5] (i) Lead [IV] oxide and concentrated hydrochloric acid on heating. (ii) Lead [II] oxide [heated] and ammonia. (iii) Lead nitrate on thermal decomposition. (iv) Lead hydroxide and dilute nitric acid. (v) Lead nitrate and ammonium hydroxide.

SECTION - B Attempt any four questions

Q2. (a) Choose the correct word or phrases from the brackets to complete the following sentences. (i) Heating sulphur with concentrated nitric acid produces —— [sulphur dioxide, nitrogen dioxide.

sulphuric acid] as the oxidised product. (ii) Heating sulphur with concentrated sulphuric acid produces —— [sulphur dioxide, nitrogen dioxide,

sulphuric acid] as the oxidised product. (iii) Ammonia gas reacts with sulphuric acid to give. [ammonium sulphate and water, tetrammine

sulphate, ammonium sulphate]. (iv) Thermal decomposition of nitric acid results in formation of two gases ——’- [one acidic and one neutral, both acidic, both neutral]. [4] (b) Give correctly balanced equations for each of the reactions mentioned in (a) (i) to (iv) above. [4] (c) Write a balanced equation for the thermal dissociation reaction of: (i) An acidic gas. (ii) A salt obtained by reaction between a basic gas and an acid. Q3. (a) (i) What is the purpose of the Contact process. (ii) State the catalyst preferred for converting sulphur dioxide to sulphur trioxide in the above process. (iii) Give the balanced equation for the above conversion. (iv) State the promoter used in the above conversion. (v) State why the product formed in the above conversion is dissolved in concentrated acid and not in

water. (vi) Write a balanced equation for the conversion of pyrosulphuric acid to sulphuric acid. [6] (b) Using dilute sulphuric acid how would you obtain: (i) A neutral gas. (ii) An acidic gas which has no effect on lime water. [2] (c) Give reasons for the following: (i) Ammonium Hydroxide is used in Analytical Chemistry (ii) Hydrogen sulphide gas is used as an analytical reagent. Q4. (a) Metallic oxides are reduced to metals by electrolysis, use of reducing agents or by thermal

decomposition. . . (i) Name a metal other than sodium, potassium, calcium or aluminium extracted by electrolysis of its

fused salt. (ii) What is Electrorefining? (iii) Write a balanced equation for the reduction of a metallic oxide with a suitable reducing agent. (iv) Give a reason why oxides of mercury and silver are reduced to metals by thermal decomposition of

their oxides.

TIWARI TUTORIALS

(v) Give a balanced equation for thermal decomposition of the nitrate of silver. (b) Give uses following metals: [4] (i) Zinc . (ii) Aluminium . (iii) Steel . (iv) Magnecium.. (c) Give al1 balanced equation for conversion of the hydroxide of the metal in period-3, group 13[IIIA] to its

respective oxide by thermal decomposition. [1] Q5. (a) Calculate purity of impure Mg , if one gram impure sample gave 298.6 cc of hydrogenat STP on reaction

with dilute sulphuric acid .[Mg=24,H=1,S=32] [5] (b) Wishing soda crystals are heated strongly till its loses’ all its water of crystallization If 9.32 g. of

washing soda on heatmg leaves 5.72 g. of the anhydrous salt, determine the formula of the hydrated salt. [Na = 23, C = 12,.0 = 16, H = 1] [5]

Q6. (a) Alkanes on oxidation give the corresponding alcohol which on further oxidation give the corresponding

aldehyde and acid respectively. (i) Give the structural formula of the corresponding alcohol, aldehyde and ad­formed as oxidation

products of ethane. (ii) Give the balanced equation for the incomplete combustion of ethane.

[4] (b) Explain the following terms with suitable examples. (i) Isomerism. (ii) Pyrolysis.

[2] (c) Give balanced equations for the following conversions. (i) Ethene to ethylene dibromide. (ii) Ethyne to

bromoethene. [2] (d) Give the condensed strucrural formula of - (i) The lcohol whose ‘name is derived from the corresponding alkane - ethane. (ii) The carboxylic acid whose name is derived from the corresponding alkane - propane. [2] Q7. (a) (i) What are ‘periods’ and ‘groups’ of a Periodic Table. (ii) Name the eight elements of Period-3 of the Modern Periodic Table in increasing order of their

atomic numbers: . (iii) Give a reason why elements of group 17[VII A] have similar chemical properties. (iv) State the position of the following elements in the periodic table. [7] (1) Alkali metals (2) Transition elements (3) Actinide series (4) Inert gases [7] (b) (i) Explain the term ‘atomic size’ of an element. (ii) State the factors which affect the atomic size of an element. (iii) State with reasons the trends in atomic size on moving down a group of the Periodic

Table. [3]

SECTION - A Q1. (a) Answer the following questions relating your answer only to the elements given in the list below: Mercury, sodium, iron, copper, silver, carbon, phosphorus, platinum, sulphur. (i) The element which forms a carbonate stable to heat. (ii) The element which form a nitrate which leaves a residue, of the same element on thermal

decomposition. (iii) The element which forms a mixed oxide on heating in air. (iv) The element which forms a neutral and an acidic oxide.

9.30 to 10 pm Have dinner 10 to 11.30 pm Solve following FULL LENGTH paper

TEST PAPER Section I is compulsory and attempt any four questions from Section II.

The intended marks for questions or parts of questions, are given in bracket [ ]

TIWARI TUTORIALS

(v) The element above hydrogen in the activity series. (vi) Write the balanced equation for the reaction occurring between a metallic element given above and

an acid which results in liberation of sulphur dioxide. (vii) The element which occurs in the free metallic form. [7] (b) Narne the term defined as follows: (i) Hydrocarbons containing a single carbon-carbon covalent bond (ii) Method of preparation of a salt from two elements. (iii) The process due to which hydrogen ions of an acid react completely with hydroxyl ions of a base to

give salt and water only. (iv) The formation of an oxide coating on aluminium on reaction with fuming nitric acid, which renders

it inactive. [4] (c) (i) Two volumes of ammonia are formed when one volume of nitrogen combines with three volumes of

hydrogen. State the Law which illustrates the given statement. (ii) State Avogadro’s Law and Gay Lussac’sLawof combining volumes. (iii) Potassium chlorate on thermal decomposition gives potassium chloride and oxygen gas. Calculate

the weight of potassium chlorate required to release 0.65 moles of oxygen at s.t.p. [K = 39, Cl = 35.5, 0 = 16] . Ans. 53.08 g.

(iv) A compound contains calcium, carbon and nitrogen only. The percentage of calcium and carbon in the compound is in the ratio 10 : 3 and-nitrogen is 35%: by mass. Determine its empirical formula. [Ca= 40, C = 12, N = 14] Ans.CaCN2

(v) State which has the least number of molecules among 2 g. of each of the following oxides: Nitric oxide, Nitrous oxide, Nitrogen dioxide. [N = 11, 0 = 16] Ans. Nitrogen dioxide [10]

(d) Rewrite each incorrect statement, correctly in full. (i) Empirical formula is the formula of a compound which represents the actual number of ions of each

element present in an atom of the compound. (ii) Ionisation potential decreases across a period on moving from left to right in a Periodic Table, since

the nuclear charge on the atom decreases and the atomic radii of the atom increases accordingly. (iii) Charge separation takes place in polar covalent compound and the atom which attracts electrons

more strongly acquired a positive charge. (iv) During electroplating of an article with silver, silver sulphate is preferred as the electrolyte, and the

article to be electroplated is placed either at the cathode or at the anode. (v) Pure water is a weak electrolyte and hence acidified with dilute hydrochloric acid. (vi) Copper reacts with dilute nitric acid on heating evolving nitrogen dioxide gas. The gas is also

liberated when magnesium reacts with cold, very dilute nitric acid. (e) Select the cotrect answer from the multiple choices A,B,C& D for the following statements. (i) Dilute sulphuric acid can be distinguished from dilute. nitric acid using: A : dilute hydrochloric acid B : sodium hydroxide C : barium chloride solution D : lead sulphate. (ii) Aluminium oxide reacts with sodium hydroxide solution to give: A : Na2AlO2 B : NaAlO2 C: NaAlO3 D : NaAlO (iii) Ethyne reacts with ammoniacal cuprous chloride to give a: A : Red precipitate of copper chloride. B : White precipitate of copper acetylide. C : Red precipitate of copper acetylide. D : Red precipitate of copper ethylene. (iv) Sodium hydroxide solution reacts with methyl orange solution to give a A : Pink colouration B : Orange colouration C : Yellow colouration D : Colourless solution. (v) A substance ~’X’ reacts with dilute sulphuric acid on heating evolving hydrogen sulphide gas. The

anion in substance ‘X’ is a A : Sulphide B : Sulphite C : Bisulphate D : Sulphate. [5] (f) Give balanced equations for the following reactions: (i) Sodiumthiosulphate and conc.HCl.

TIWARI TUTORIALS

(ii) Aluminium chloride and sodium hydroxide solution. (iii) Concentrated hydrochloric acid and potassium permanganate. (iv) Dilute nitric acid and acidified iron [II] sulphate solution. (v) Pentachloroethane and chlorine. (vi) Cane sugar and concentrated .sulphuric acid. (vii) Aq. Ammonia and chlorine. (viii) Ammonium hydroxide and dilute sulphuric acid. [8]

SECTION - II (40 Marks) Attempt any four questions

Q2. (a) (i) Name the elements in group l[IA], 2[IIA], 15[VA], and 16[VIA] of Period-2 and Period-3 of the

Periodic Table. (ii) State the valency of each of the elements stated in (a) (i) above. (iii) Give a reason why ‘neon’ and ‘argon’ have ‘zero valency’. (iv) State the character trends of the type of oxides of elements of Period-3 of the Periodic Table on

moving from left to right in a period. (b) Give one example of each of the following: (i) A radioactive element. (ii) A transition element. (iii) An inner transition element. (iv) An alkali earth metal. (c) (i) State the factors influencing the metallic and non-metallic character of elements in a Periodic Table. (ii) State the trend in metallic and non-metallic character across a period from left to right in a Periodic

Table & down a group of a period. Q3. (a) What would you add to concentrated sulphuric acid to obtain the following: (i) Hydrochloric acid. (ii) Nitric acid. (iii) Sulphur. (iv) Ethene. (b) Give reasons for the following: (i) Sulphur dioxide is called ‘sulphurous anhydride’. (ii) Sulphuric acid forms an acid salt and a normal salt with an alkali. [2] (c) Give balanced equations for the following conversions: (i) Carbon to carbonic acid using an acid. (ii) Sulphur to sulphuric acid using an acid. (iii) HI to Iodine using conc. nitric acid (iv) Hydrogen sulphide to sulpher using conc. nitric acid [4] Q4. (a) State the correct answer from the multiple choice of answers as per the instruction in bracket. (i) The organic compound which does not form an isomer. [ethane, pentane, I-butene]. (ii) Ethane, propylene, butyne-I, formaldehyde, ethyne. [the organic compound which is not a hydrocarbon]. (iii) Ethyne, ethene, ethane, propene, propyne. [the paraffin] (iv) Ethane, ethanol, ethyne, acetylene, propyne [the hydroxyl derivative of an alkane]. (v) C2H6, C3H6, C3H4, CH4, C2H4· [the unsaturated hydrocarbon containing a double bond]. [5] (b) Give balanced equations for the following conversions. (i) Ethyne to ethene. (ii) Methanol to sodium methoxide. [2] (c) State which of the following - acetic acid, methanol, ethanol is used in/ as- (i) Food industry for preserving and flavouring food. (ii) In thermometers and spirit levels (iii) Solvent for paints .and varnishes [3]

TIWARI TUTORIALS

Q5. (a) Narne the following: (i) A metal which is not very malleable. (ii) A non-metal having high melting and boiling point. (iii) A metal having density less than water. (iv) A metal which is a poor conductor of electricity. (v) A metal which is present in the alloy type metal but not in gun metal: (vi) A metal occurring in the combined form in ‘Fluorspar’. [4] (b) State the term used for each of the following: (i) The rocky impurities associated with the ore. (ii) The process of heating the concentrated ore in presence of excess air before it is reduced to the

metal. [2] (c) ‘Give balanced equations for the following conversions A, B, C & D: Al2O3.2H2O NaAlO2 Al(OH)3 Al2O3 Al [4] Q6. (a) Narne the following: (i) The gaseous product obtained when hydrogen sulphide reacts with nitric acid. (ii) Gaseous product when conc.hydrochloric acid reacts with mangnese dioxide (b) Give balanced equations for the reactions in (a) (i) & (ii) above. [2] (c) Give a balanced equation in each case for following reactions pertaining to the respective properties of

the substances concerned: (i) Ammonia as a reducing agent. (ii) Ammonia as reducing agent. (iii) Nitric acid as an oxidising agent. [3] (d) Give reasons for the following: . (i) Ammonia reacts with acids to give ammonium salts. (ii) Why temperature is less than 200 during lab method of HCl. (iii) Aqueous hydrogen chloride solution is an electrolyte but a solution of hydrogen chloride in an organic solvent is a non-electrolyte. [3] Q7. (a) Calculate the molecular formula of an organic compound whose empirical formula is C2H6O and vapour

density is 23. Ans. C2H6O . [3] (b) A mixture of butane [C4HlO] and water gas [CO and H2] are mixed together with oxygen gas and ignited.

The amounts of butane, water gas and oxygen used are 10 cc., 50 cc. and 1000 cc. respectively. Calculate the composition of .the residual mixture, if all measurements are made under the same conditions of temperature and pressure. Ans. CO2 = 45 CC., O2 = 910 cc. [5]

(c) Calculate the percentage of oxygen in calcium phosphate. [Ca = 40, P = 31, O = 16] Ans. 41.29% [2]

11.30 to 12 am Solve problems of both papers TAKE SOUND SLEEP OF 6 HRS. WISH YOU ALL THE VERY BEST FOR HIGHLY SCORING ICSE 2015