significant figures and scientific notation...
TRANSCRIPT
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Significant Figures and Scientific Notation Name __________________________
Remember the rules: 1. All non-zero digits are significant. 2. Sandwiched zeros are significant. 3. Zeros to the right of a decimal and to the right of a non-zero digit are significant. 4. Zeros between a non-zero digit and a decimal in numbers greater than 1 are significant. How many significant figures? 1. 9.07 _______ 6. 9.23 x 105______ 11. 1.00 ______ 2. 1450 _______ 7. 0.03 _______ 12. 1.020 _______ 3. 12 _______ 8. 0.003 _______ 13. 0.02 _______ 4. 1200 _______ 9. 1.003 _______ 14. 0.00300 _______ 5. 1200. _______ 10. 3.00 x 10-8_______ 15. 100 _______ Write in scientific notation and keep the same number of significant figures: 16. 400,003 ___________ 21. 0.00450 ___________ 26. 100 ___________ 17. 0.00007 ___________ 22. 156,000 ___________ 27. 100. ___________ 18. 19000 ___________ 23. 123456 ___________ 28. 1000 _____________ 19. 420034 ___________ 24. 0.00100 ___________ 29. 1000. ___________ 20. 422000 ___________ 25. 0.001 ___________ 30. 100.1 ___________ Write in standard notation and keep the same number of significant figures: 31. 3.1 x 104 _____________ 36. 2.90 x 10-4 __________ 32. 5.506 x 109 _____________ 37. 1.45 x 106 __________ 33. 2.48 x 103 _____________ 38. 9.9 x 10-5 __________ 34. 1.0 x 10-4 _____________ 39. 1.00 x 102 __________ 35. 1.000 x 10-3 _____________ 40. 1.0000 x 104 __________ Round to 3 significant figures: Round to 4 significant figures: 41. 6080.4 _________ 42. 6080.4 _____________ 43. 0.003008 _______ 44. 4.50049 x 10-4 __________
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Significant Figures and Calculator Practice Name ________________________ Use your calculator. Round to the correct number of significant figures. Include the correct units if units appear. Put your answer in the blank. _____________ 1. (2.3cm)(4.007cm) =
_____________ 2. 6.75 m + 5.003 m =
_____________ 3. 45.0 cm - 9.2 cm =
_____________ 4. (2.25 x 109) (4.6) =
_____________ 5. 22.2 g + 750.00 g =
_____________ 6. 4.794 g / 4.98 cm3=
_____________ 7. (65 x 28 x 1.22) / (5.5 x 47 x 13.9)=
_____________ 8. 4.90 mm + 34.7 mm =
_____________ 9. (8.85 x 104)(4229) =
_____________ 10. (75cm)(1.23 x 105cm) =
_____________ 11. 4100g / 55.5 mL=
_____________ 12. 400 x 600 =
_____________ 13. (8.9 cm x 4.0 cm x 122 cm) / (56 cm x 0.0045 cm)=
_____________ 14. 400. m3 / 3.07 x 10-5m =
_____________ 15. (16.0)(1.48 x 1010) =
_____________ 16. 1289.2 x 109 / (346 x 6.890 x 10-4)=
_____________ 17. 3.499 x 1013 / 349.00=
_____________ 18. 50.0 g – 25.59 g =
_____________ 19. (1.298 x 10-5 x 1.399 x 10-16) / (135 x 1.59 x 10-7) =
_____________ 20. 40.5 x 340 x 544 / 6044=
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Dimensional Analysis (one step) Name ______________________________ Use factor label method. Show the correct units on every step. Round to the correct number of significant figures. Put answer in the blank. 1. _____________ How many minutes are there in 5 weeks if one week is equal to 10080 minutes? 2. _____________ Convert 44.6 g to milligrams. 3. _____________ Convert 33.4 milliliters to liters. 4. _____________ If 1 gallon is equal to 3785 ml, how many gallons equal 2300 mL? 5. _____________ How many grams is a person who weighs 134 pounds if one pound is equal to 454g? 6. _____________ If candy bars are 3 for one dollar, how much money will you need to by 46 candy bars? 7. _____________ Convert 44.56 kg to g. 8. _____________ How many drops of water will fit in a 50.0 mL flask if 1 mL is equal to 15.4 drops?
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Dimensional Analysis (Two steps) Name ________________________ 1. _____________ Convert 3.490 km to m and express in scientific notation. (1 step) 2. _____________ How many milligrams are in 34 kg? 3. _____________ What is the length of a football field in cm is there are 2.54 cm in an inch and 36 inches in a yard? 4. _____________ What is the circumference of a ball in cm if it has a circumference of 2.1 feet? 5. _____________ Convert 3.45 cm to km and express in scientific notation. 6. _____________ If 4.003 g of helium contains 6.02 x 1023 atoms, how many atoms are in 6.95 g of helium? (1 step) 7. _____________ If light travels at the speed of 3.00 x 108 m/s, how far does light travel in 2.05 minutes? 8. _____________ Convert 75 cm to feet. 9. _____________ What volume will be occupied by 7.0 kg of helium if 4.003 g of helium occupies 22.4 L?
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Name ________________________
Show your work using the three steps for working problems with a formula. Answer should be boxed with correct units and correct number of sig figs. 1. _____________ Calculate the density of a marble if 5 marbles displace the water in a graduated cylinder from 15.5 mL to 19.8 mL and the mass of the five marbles is 8.97 g. 2. _____________ What is the mass of a block that measures 6.7 cm by 6.8 cm by 4.3 cm and has a density of 22.29 g/cm3? 3. _____________ What is the volume of a rock that has a mass of 22.48 g and a density of 7.11 g/mL? 4. _____________ Twenty five paper clips are dropped into a graduated cylinder and the water level rises from 10.8 mL to 12.2 mL. If the density of the paper clips is 7.87 g/mL, what is the mass of the 25 paper clips? What is the mass of one paper clip?
5. _____________ Twelve quarters displace the water in a graduated cylinder from 15.0 mL to 21.2 mL. If the mass of the quarters is 60.66 g, what is the density of the 12 quarters? What is the density of one quarter?
6. _____________ A tennis ball can is 18.5 cm tall and has a diameter of 9.8 cm. If you filled the can with water, which has a density of 1.00 g/cm3, how many grams of water would you have?
7. _____________ A block of wood with a density of 0.548 g/cm3 has a mass of 34.49g. If two dimensions of the block are 2.5 cm and 7.8 cm, what is the 3rd dimension?
8. _____________ Copper has a density of 8.96 g/cm3. If a thin sheet of copper measures 5.5 cm by 5.5 cm and has a mass of 12.96 g, what is its thickness?
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Name ________________________________
Ion Symbol Atomic number Mass number Protons Neutrons Electrons Iodide I-1 127 53 54
Cl-1 35 17
Hydrogen 1 1 0
Br-1 35 46 35 79 36
B+3 5 11
Oxide O-2 16 8 Nitride 7 7 10
Aluminum Al+3 27 10
Fe+2 56 26 24
Cu+1 29 34 63 29 27
Element Isotope notation Atomic number Mass number Protons Neutrons Electrons
Carbon 6 14
O 8 10
Potassium 19 20
19 41
197Au
Tin Sn 50 68
Zinc 64 30
66 30 68 30
Cobalt Co 27 32
Boron 5 6
10 5
56Fe
26 28
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Average Atomic Mass Name _______________________________ 1. Calculate the average atomic mass for neon if its abundance in nature is 90.5% neon-20, 0.3% neon-21, and 9.2% neon-22. 2. Only two isotopes of copper occur naturally. 63Cu (mass = 62.9298 amu; abundance 69.09%) and 65Cu (mass = 64.9278 amu; abundance 30.91 %). Calcualte the average atomic mass of copper. 3. Magnesium consists of three naturally occurring isotopes. The percent abundance of these isotopes is as follows: 24Mg (78.70%), 25Mg (10.13%), and 26Mg (11.7%). The average atomic mass of the three isotopes is 24.3050 amu. If the atomic mass of 25Mg is 24.98584 amu, and 26Mg is 25.98259 amu, calculate the actual atomic mass of 24Mg. 4. Naturally occurring chlorine is 75.53 percent 35Cl which has an atomic mass of 34.969 amu, and 24.47 percent 37Cl which has an atomic mass of 36.966 amu. Calculate the average atomic mass.
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Mole problems with elements Name_________________________________ Use dimensional analysis to solve the following problems. Show your work, use sig figs, and include units to get credit. 1. _________________ How many grams of zinc are in 5.67 moles? 2. _________________ How many atoms are in 0.415 grams of sulfur? 3. _________________ What is the mass of 1000. gold atoms? 4. _________________ How many moles are equal to 1000. gold atoms? 5. _________________ How many grams are in 2.93 x 10-2 moles of calcium? 6. _________________ How many atoms are in 45.876 grams of helium? 7. _________________ How many moles are equal to 5.098 x 1023 atoms of hydrogen? 8. _________________ 57.90 grams of chromium is equal to how many moles? 9. _________________ 8.954 moles of barium is equal to how many atoms? 10. _________________ 1.2044 x 1024 atoms is equal to how many moles of lithium? 11. _________________ How many grams of copper are in 7.055 moles?
12. _________________ How many moles of nickel are equal to 2.04 x 10-4 grams?
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Name ______________________________ Write the orbital notation for the following elements: 1. Carbon
2. Lithium
3. Chlorine
4. Sulfur Write the full electron configuration notation for the following elements: 5. Potassium _____________________________________________________
6. Magnesium _____________________________________________________
7. Arsenic _____________________________________________________
8. Silicon _____________________________________________________
9. Manganese _____________________________________________________
10. Antimony _____________________________________________________ Write the shorthand electron configuration notation for the following elements: 11. Cesium _____________________________________________________
12. Bromine _____________________________________________________
13. Oxygen _____________________________________________________
14. Xenon _____________________________________________________
15. Promethium _____________________________________________________
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Fill in table with appropriate information: Name ____________________________
Barium
[Kr] 5s24d105p4
Antimony
Indium
[He] 2s22p5
5 2
Germanium
Show full electron configuration notation for the following ions. 1. Na+1 __________________________________________________ 2. Cl-1 ___________________________________________________ 3. N-3 ___________________________________________________ 4. O-2 ___________________________________________________ 5. C-4 ___________________________________________________ What do you notice about the final energy levels?
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Ionic Nomenclature Name __________________________ Write the correct chemical formula for the ionic compounds.
Write the correct names for the following ionic compounds.
1. sodium phosphide __________
21. CdO _______________________________
2. zinc phosphide __________
22. LiBr _______________________________
3. strontium oxide __________
23. PbO2 ______________________________
4. magnesium phosphide __________
24. ZnO _______________________________
5. aluminum oxide __________
25. BaS _______________________________
6. potassium sulfide __________
26. ZnCl2 _______________________________
7. beryllium chloride __________
27. CoI2 _______________________________
8. mercury(II) phosphide __________
28. Ag3N _______________________________
9. calcium iodide __________
29. CuCl2 _______________________________
10. magnesium iodide __________
30. FeI3 _______________________________
11. gold(III) oxide __________
31. Fe3N2 ______________________________
12. magnesium oxide __________
32. MgI2 _______________________________
13. silver oxide __________
33. LiF _______________________________
14. barium sulfide __________
34. BaBr2 ______________________________
15. sodium nitride __________
35. CaCl2 ______________________________
16. silver nitride __________
36. CoN _______________________________
17. iron(II) sulfide __________
37. CsCl _______________________________
18. lithium fluoride __________
38. AuN _______________________________
19. manganese(III) oxide _________
39. SnS _______________________________
20. magnesium chloride __________ 40. AgCl _______________________________
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Name ______________________________
Compound made of…. Cation Anion Formula Compound Name # of atoms in compound
Sodium and iodine
Lithium and phosphorus
Tin(IV) and chlorine
Copper(II) and carbonate
Ammonium and nitrate
Lead(II) and phosphate
Magnesium and hydroxide
Silver and sulfur
Barium and acetate
Fluorine and manganese(II)
Chromium(III) and nitrate
Sulfate and iron(III)
Calcium and chlorate
Chlorine and magnesium
Aluminum and nitrate
Iron(III) and carbonate
Lithium and sulfate
Strontium and carbonate
Phosphate and iron(III)
Fluorine and ammonium
Calcium and hydroxide
Tin(II) and sulfate
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Molecular Nomenclature
Write the formulas for the following molecular compounds.
Name ____________________________
1. dichlorine monoxide ____________
2. chlorine trifluoride ___________
3. phosphorus pentachloride ____________
4. carbon dioxide ____________
5. silicon dioxide ____________
6. phosphorus tribromide ____________
7. carbon monoxide ____________
8. pentaphosphorus decoxide ____________
9. dinitrogen pentoxide ____________
10. diphosphorus trioxide ____________
11. disulfur trioxide ____________
Write the name for the following molecular compounds. 12. N2O4 _______________________
13. PCl3 _______________________
14. N2O _______________________
15. SiF4 _______________________
16. P2S3 _______________________
17. P2O5 _______________________
18. SiO2 _______________________
19. B2O3 _______________________
20. P5O10 _______________________
21. BF3 _______________________
22. N2O5 _______________________
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Acid Nomenclature Name __________________________ If an ionic compound begins with hydrogen then it is an acid. It will dissociate in water. These compounds can be given an “acid name”. For example, we have learned the following names:
o HCl is hydrogen chloride o HNO3 is hydrogen nitrate o H2SO3 is hydrogen sulfite
Notice that the endings for these 3 ionic salts are “ide”, “ate” and “ite”. We use these endings to determine the acid name as follows. Drop hydrogen out of the name and drop the ending.
o If the name ends in “ide” then it becomes hydro______ic acid. o If the name ends in “ate” then it becomes ______ic acid. o If the name ends in “ite” then it becomes ______ous acid.
So for the examples above:
Formula Ionic name Acid name HCl Hydrogen chloride Hydrochloric acid HNO3 Hydrogen nitrate Nitric acid H2SO3 Hydrogen sulfite Sulfurous acid (sulfous acid) 1. HClO 2. HClO2 3. HClO3 4. HBr 5. H2SO4 6. HMnO4 7. H2CO3 8. H3PO4 9. HBrO3 10. H2C2O4
Write the formula for the following acids: 11. hydrofluoric acid ______________________________________ 12. sulfuric acid ________________________________________ 13. hydroiodic acid ________________________________________ 14. hydrobromic acid _______________________________________ 15. hypochlorous acid ________________________________________ 16. nitrous acid __________________________________________ 17. acetic acid ___________________________________________ 18. hydrosulfuric acid _________________________________________
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Mole Problems with Compounds Name______________________________
For each compound, write the formula in the first blank and the molar mass in the second. 1. Sodium iodide ___________________ ___________________ 2. Calcium chloride ___________________ ___________________ 3. Magnesium hypochlorite ___________________ ___________________ Solve each molar conversion problem and put your answer in the blank. Show your work!!! 4. _______________ How many molecules are in 10.8 grams of C12H22O11?
5. _______________ What is the mass of 0.95 moles of potassium hydroxide?
6. _______________ How many formula units are equal to 55.67 g of KMnO4?
7. _______________ What is the mass of 5.23 x 1021 formula units of Au2(SO4)3?
8. _______________ How many formula units are in 25.5 g of iron (III) hydroxide?
9. _______________ What is the mass of 0.578 moles of sodium oxide?
10. _______________ How many formula units are equal to 6.78 x 10-3 moles of cadmium nitride?
11. _______________ What is the mass of 2.45 x 1022 formula units of nickel (III) iodide?
12. _______________ How many moles are equal to 6.78 x 104 g of iron (III) sulfide?
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Name ____________________________Solve the following problems and put your answer in the blank. 1. _______________ What is the empirical formula of a compound that is 29.00% calcium, 23.56% sulfur, and 47.44% oxygen? 2. _______________ What is the empirical formula of a compound that is 80.0% carbon and 20.0% hydrogen if it has a molar mass of 30.0 grams? 3. _______________ What is the molecular formula of the compound in problem 2? 4. _______________ What is the empirical formula of a compound that is 24.3% carbon, 4.1% hydrogen, and 71.6% chlorine? 5. _______________ What is the molecular formula of the compound in problem 4 if its molar mass is 98.9 grams? 7. _______________ Ascorbic acid (vitamin C) contains 40.92% carbon, 4.58% hydrogen, and 54.50% O by mass. What is the empirical formula for ascorbic acid?
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Name ____________________________ Give the oxidation numbers of all the elements in the following molecules and ions: 1. SO 2. SO2 3. SO3 4. SO3
2- 5. SO4
2- 6. N2O 7. NO 8. NO2 9. N2O4 10. N2O5 11. H2S 12. H2SO4
13. HPO3 14. H3PO 15. H3PO2 16. H4P2O7
Give oxidation numbers for the underlined atoms in these molecules and ions: 17. Cs2O 18. PtCl62- 19. CaI2 20. SnF2 21. Al2O3 22. ClF3 23. H3AsO3 24. SbF6
-
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Balancing Equations Name __________________________ Write a balanced equation by using coefficients. 1. __ N2 + __ H2 → __NH3 2. __ KClO3 → __ KCl + __ O2 3. __ NaCl + __ F2 → __ NaF + __ Cl2 4. __ H2 + __ O2 → __ H2O 5. __ AgNO3 + __ MgCl2 → __ AgCl + __ Mg(NO3)2 6. __ AlBr3 + __ K2SO4 → __ KBr + __ Al2(SO4)3 7. __ CH4 + __ O2 → __ CO2 + __ H2O 8. __ C3H8 + __ O2 → __ CO2 + __ H2O 9. __ C8H18 + __ O2 → __ CO2 + __ H2O
10. __ FeCl3 + __ NaOH → __ Fe(OH)3 + __ NaCl 11. __ P + __ O2 → __ P2O5 12. __ Na + __ H2O → __ NaOH + __ H2 13. __ Ag2O → __ Ag + __ O2 14. __ S8 + __ O2 → __ SO3 15. __ CO2 + __ H2O → __ C6H12O6 + __ O2 16. __ HCl + __ CaCO3 → __ CaCl2 + __ H2O + __ CO2
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Write and balance the following equations: 1. Hydrogen plus oxygen yield water. 2. Nitrogen plus hydrogen yield ammonia. 3. Aluminum bromide plus chlorine yield aluminum chloride and bromine. 4. Hydrochloric acid plus sodium hydroxide yield sodium chloride plus water. 5. Iron plus lead (II) sulfate react forming iron (II) sulfate plus lead. 6. Potassium chlorate when heated produces potassium chloride plus oxygen gas. 7. Sodium oxide combines with water to make sodium hydroxide. 8. Potassium iodide reacts with bromine forming potassium bromide plus iodine. 9. Sodium phosphate reacts with calcium nitrate to produce sodium nitrate plus calcium phosphate. 10. Zinc reacts with iron (II) chloride yielding zinc chloride plus iron precipitate. 11. Ammonium carbonate and magnesium sulfate react to yield ammonium sulfate plus magnesium carbonate. 12. Phosphoric acid plus calcium hydroxide react forming solid calcium phosphate plus water. 13. Nitrogen gas plus oxygen gas react and form dinitrogen pentoxide. 14. Copper (II) nitrate and ammonium hydroxide yield copper (II) hydroxide and ammonium nitrate. Write the word equation from the following balanced chemical equations. 15. 2NaCl + F2(g) → 2NaF + Cl2(g) 16. 2NaOH (aq) + CO2 (g) → Na2CO3 +H2O
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Identify the reaction as either synthesis or decomposition, and then use your notes to complete and balance the equations. 1. Potassium chlorate → 2. Calcium and oxygen →
3. sodium chlorate → 4. calcium hydroxide → 5. chlorine plus calcium → 6. beryllium oxide plus water →
7. barium nitride → 8. magnesium oxide plus water → 9. water → 10. sodium carbonate → 11. sulfuric acid →
12. lithium chlorate → Write 4 additional synthesis or decomposition reactions. 13. 14. 15. 16.
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Single Replacement Rxns Name ____________________________
Use the activity series to determine if the following single replacement reactions occur. If they do, write the equation and balance. If the reaction does not occur, write the reactants, the yield sign, and “No Reaction”. 1. calcium and hydrochloric acid 2. silver and tin(IV) bromide 3. zinc and copper (II) nitrite 4. sodium and silver sulfide 5. bromine and gold(I) chloride 6. chromium (III) oxide and potassium 7. lithium and sulfuric acid 8. mercury and nickel(II) carbonate 9. fluorine and potassium chloride 10. barium iodide and bromine
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Name ____________________________ Write the products of the following double replacement reactions. Both reactants will be in aqueous solutions. Use the solubility chart to determine if any of the products are precipitates. If so, mark them with a (s). Mark all soluble products with (aq). If a gaseous product forms, mark it with a (g). 1. silver nitrate + calcium iodide
2. barium hydroxide + sodium sulfate
3. magnesium iodide + sodium carbonate
4. nitric acid + lithium hydroxide
5. phosphoric acid + magnesium acetate
6. ammonium chloride + calcium hydroxide
7. sodium carbonate + hydrochloric acid
8. lead (II) nitrate + sodium chloride
9. lithium sulfite + hydrobromic acid
10. magnesium chloride + cesium sulfate
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Reaction predictions: All types Name ____________________________
Directions:
o Look at reactants given.
o Determine the type of reaction that is occurring. Write (s, d, c, sr, or dr) in the left margin.
o Predict all products.
o Write a balanced chemical equation for the reaction.
1. aluminum + oxygen
2. potassium carbonate + barium chloride
3. calcium chloride + nitric acid
4. propane (C3H8) and oxygen
5. barium chloride and iodine
6. ammonium sulfide and lead (II) nitrate
7. calcium carbonate
8. sodium carbonate
9. iron and copper (II) nitrate
10. magnesium bromide
11. bromine and calcium iodide
12. calcium hydroxide
13. sodium and water
24. strontium oxide and water
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Net Ionic Problems Name ____________________________________
Write a balanced equation, the total ionic and net ionic equation. Box your net ionic equation. 1. Solutions of calcium carbonate and hydrochloric acid are mixed. 2. Solid iron reacts with a solution of silver nitrate. 3. A solution of lead (II) nitrate is added to hydrochloric acid. 4. Sodium hydroxide is mixed with a solution of nitric acid. 5. Lithium is added to water. 6. Chlorine gas reacts with a solution of potassium iodide.
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STOICHIOMETRY- Mole to Mole Name ____________________________ Write and balance the equations. Calculate the number of moles. 1. a. Sodium reacts with water to form sodium hydroxide and hydrogen gas. b. How many moles of hydrogen gas will form if 0.35 moles of Na reacts with an excess of water? 2. a. Double replacement reaction between phosphoric acid and potassium carbonate. b. How many moles of phosphoric acid are needed to react with 1.248 moles of potassium carbonate? 3. a. Ethanol, C2H5OH, is produced when glucose, C6H12O6 ferments. The other product is carbon dioxide. b. How many moles of glucose must ferment to produce 7.5 moles of ethanol? c. How many moles of carbon dioxide will be produced as a by product? 4. a. Ammonium nitrate decomposes into nitrogen gas, water, and oxygen gas. b. How many moles of oxygen gas are produced when 8.14 moles of ammonium nitrate decompose?
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Name ____________________________
Show all work: 1. a. Write the balanced equation for the decomposition of sugar, C12H22O11, into carbon and water. b. How many moles of water would be produced if you started with one mole of sugar? c. How many moles of water would be produced if you started with 12 moles of sugar? d. How many moles of sugar would you have to start with to end up with 8.7 moles of carbon? e. If you had 120 g of sugar and all of it decomposed, how many moles of water would be produced? f. If you produced 15 g of carbon, how many moles of water would also be produced? g. How many moles of carbon would be produced if you started with 2 grams of sugar?
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Name ______________________
1. a. Aluminum is strongly heated with oxygen. Equation: b. How many moles of oxygen are needed to react with 3.46 g of aluminum? c. How many grams of aluminum oxide will form? 2. a. Calcium carbonate reacts with sulfur dioxide and oxygen to produce calcium sulfate and carbon dioxide. Equation: b. How many moles of calcium sulfate will be produced if 15.50 g of calcium carbonate reacts with an excess of sulfur dioxide and oxygen? c. How many grams of O2 will react with 15.50 g of calcium carbonate? 3. a. C5H11 reacts with oxygen in a combustion reaction. Equation: b. How many grams of C5H11 must be burned to produce 1.25 grams of water?
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AND MORE STOICHIOMETRY Name ____________________________ 1. How many moles of hydrogen and how many moles of oxygen form when 4.4 moles of water decompose? 2. What is the % yield if 3.12 g of magnesium reacts with phosphoric acid to form 14.15 g of magnesium phosphate? 3. What is the limiting reagent when 4.7 g of iron and 8.94 g of oxygen react to form iron(III) oxide? 4. Calcium bromide reacts with 5.100 g of aluminum oxide in a double replacement reaction. How much calcium bromide must be present for all of the aluminum oxide to react? 5. What is the limiting reagent when 7.4 moles of calcium reacts with 10.6 g of water to produce calcium hydroxide and hydrogen? 6. How many grams of aluminum nitrate will be produced if 5.78 moles of aluminum react with an excess of nitric acid. 7. Zinc chloride is produced from the reaction between zinc and chlorine gas. How many grams of zinc and how many grams of chlorine are needed to produce 65.0 g of zinc chloride if the reaction goes to completion? 8. Copper replaces silver in the reaction between copper and silver nitrate to form copper(II) nitrate and silver. How many grams of silver will form if 4.6 moles of copper are allowed to react with an excess of silver nitrate?
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LIMITING REACTANTS Name ____________________________ The compound “cisplatin” PtCl2(NH3)2 is effective in treating some types of cancer. It can be synthesized using the following reaction:
K2PtCl4 + 2NH3 → 2KCl + PtCl2(NH3)2 1. How much cisplatin can be produced from 2.50 grams of K2PtCl4, if there is plenty of NH3? 2. Exactly how much NH3 would be needed to react with those 2.50 grams of K2PtCl4? 3. If we started out with 3.50 grams of K2PtCl4 and 10.9 grams of ammonia, which reactant would be the limiting reactant? 4. How much cisplatin would be produced? 5. Suppose a researcher needs exactly 5.00 grams of cisplatin for an experiment. How much K2PtCl4 would she need to start with, assuming she has an excess of ammonia?
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Name ____________________________F O K Al
F- O2- K+ Al3+
F2 H2 HF NH3
CH4 NF3 SiF4 CS2
I2 BH3 CN- CO2
HCN (carbon in middle) CO O2 PO43-
NO3- XeF6 O3 SF6
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Name ____________________________Molecule or Ion Lewis structure Molecular geometry Polarity Hybridization (central atom)
CO2
SO42-
SiBr4
XeCl4
SeF4
H2S
CH4
SF4
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1. What will happen to the pressure of a compressed gas if the temperature is lowered? Explain WHY. 2. Why is it important not to puncture an aerosol can? Explain WHY. 3. Explain why an unopened bag of potato chips left in a car on a hot day appears to become larger. 4. If two variables have an inverse (indirect) relationship, what happens to the value of one as the value of the other increases? 5. If two variables have a direct relationship, what happens to the value of one as the value of the other is increased? 6. Label the following as being generally representative of a direct or inverse relationship.
a. Popularity of a musical group versus how hard it is to get tickets to a concert __________________ b. Number of carats a diamond weighs versus its cost __________________ c. Number of people helping versus how long it takes to clean your lab table __________________
7. What is the pressure of a fixed volume of gas at 30.0ºC if it has a pressure of 1.11 atm at 15.0ºC? 8. A fixed amount of oxygen gas is held in a 1.00 L tank at a pressure of 3.50 atm. The tank is connected to an empty 2.00 L tank by a short tube with a valve. After the valve has been opened and the oxygen is allowed to flow freely between the two tanks at a constant temperature, what is the final pressure of the system (careful on this one)? 9. Hot-air balloons rise because the hot air inside the balloon is less dense than the cooler air outside. Calculate the volume an air sample will occupy inside a balloon at 43.0ºC if it occupies 2.50 L at the outside air temperature of 22.0ºC, assuming the pressure is the same in both locations.
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Combined and Ideal Gas Laws Name ____________________________
1. A sample of nitrogen gas is stored in a 500.0 mL flask at 108 kPa and 10.0ºC. The gas is transferred to a 750.0mL flask at 21.0ºC. What is the pressure of nitrogen in the second flask? 2. The air in a dry, sealed 2-L soda bottle has a pressure of 0.998 atm at sea level and a temperature of 34.0 degrees Celsius. What will its pressure be if it is brought to a higher altitude where the temperature is 23.0 degrees Celsius? 3. A weather balloon is filled with helium that occupies a volume of 5.00 x 104 L at 0.995 atm and 32.0 degrees Celsius. After it is released, it rises to a location where the pressure is 0.720 atm and the temperature is -12.0 degrees Celsius. What is the volume of the balloon at that new location? 4. The lowest pressure achieved in a laboratory is about 1.0 x 10-15 mm Hg. How many molecules of gas are present in a 1.00 L sample at that pressure and a temperature of 22.0ºC 5. A 2.00 L flask is filled with propane gas (C3H8) at 1.00 atm and -15.0ºC. What is the mass of the propane in the flask? 6. Determine the pressure inside an old-fashioned television picture tube with a volume of 3.50 L that contains 2.00 x 10-5 g of nitrogen gas at 22.0ºC. 7. Determine how many liters 8.80 g of carbon dioxide gas would occupy at: a. STP b. 160ºC and 3.00 atm c. 288 K and 118 kPa
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Density, Dalton, and Graham’s Law
1. Propane, C3H8, is a gas commonly used as a home fuel for cooking and heating. a. Calculate the volume that 0.540 mol of propane occupies at STP. b. Think about the size of this volume compared to the amount of propane it contains. Why do you think propane is usually liquefied before it is transported? 2. Carbon monoxide is a product of incomplete combustion of fuels. Find the volume that 42 g of carbon monoxide gas occupies at STP. 3. Determine the density of chlorine gas at 22.0ºC and 1.00 atm of pressure. 4. Geraniol is a compound found in rose oil that is used in perfumes. What is the molar mass of geraniol if its vapor has a density of 0.480 g/L at a temperature of 260.0ºC and a pressure of 0.140 atm? 5. A gas diffuses 5/3 times faster than carbon dioxide. Calculate the molar mass of the gas, and determine which gas might it be from the list below. a. O2 b. N2 c. CO d. He e. CH4 6. What is the pressure exerted by some nitrogen gas collected in a tube filled with water on a day when the room temperature is 18.0 °C and the room pressure is 750.0 mmHg? [The partial pressure of water at 18 °C is 15.5 mmHg.] 7. At a given temperature, gaseous ammonia molecules (NH3) have a velocity that is _____ (greater than or less than) gaseous sulfur dioxide molecules (SO2).
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Write the formula for each of the following compounds, determine if it is a strong electrolyte and whether it will be soluble in water based on the solubility rules.
Compound Formula Strong electrolyte? (Y/N) Soluble in water (Y/N) Sodium hydroxide
Copper (II) chloride
Silver Sulfate
Potassium carbonate
Sulfuric Acid
Lead (II) nitrate
Silver chloride
Sodium acetate
Barium sulfate
Magnesium nitrate
Perchloric acid
Tin (IV) sulfide
Aluminum Phosphate
Lead (II) iodide
Sodium permanganate
Strontium Sulfate
Carbon dioxide
Hydrogen gas
Lithium Oxide
Calcium hydroxide
Hydrochloric acid
Hydrofluoric acid
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Create a graph in your notebook. Label the axes with correct scale and units. Plot the solubility of sulfur dioxide and ammonium chloride on the same graph. Use a different color to differentiate the 2 plotted lines.
Sulfur Dioxide Ammonium Chloride
Temperature (0 ºC) Solubility (g per 100
g of water)
Temperature (0 ºC) Solubility (g per 100
g of water)
0 24 0 28
20 10 20 37
40 6.1 40 46
60 4.2 60 55
80 4.1 80 66
100 4.0 100 78
Questions regarding the graph you created: 1. ________________________ Which of the two compounds is most soluble at 30 degrees Celsius?
2. ________________________ What is the solubility of sulfur dioxide at 55 degrees Celsius?
3. ________________________ Based on the graph, do you think sulfur dioxide is a solid or gas?
4. ________________________ Based on the graph, do you think ammonium chloride is a solid or a gas?
5. ________________________How much sulfur dioxide must be added to 100 grams of water to create a saturated solution at 30 degrees Celsius? 6. ________________________ at 70 Celsius, 50 grams of ammonium chloride are added to 100 grams of water. How would you describe the solution?
7. ________________________ How many grams of sulfur dioxide can be dissolved in 200 grams of water at 10 degrees Celsius?
8. ________________________ A saturated solution of ammonium chloride is prepared at 80 degrees Celsius. If the solution is cooled to 40 degrees Celsius and agitated, how much solute will precipitate out?
9. ________________________How many grams of sulfur dioxide could be dissolved in 50 grams of water at 50 degrees Celsius?
10. ________________________ 12 grams of sulfur dioxide are dissolved in 100 grams of water at 20 degrees Celsius. How would you describe the solution?
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1. Sea water contains roughly 28.0 grams of NaCl per liter. What is the molarity?
2. What is the molarity of 245.0 grams of H2SO4 dissolved into 1.00 liter of solution?
3. What is the molarity of 5.30 grams of NaOH dissolved in 750.0 mL of solution?
4. How many grams of Na2CO3 are in 10.0 mL of a 2.0 M solution?
5. Calculate the molality of 25.0 grams of KBr dissolved in 750.0 grams of pure water.
6. 89.0 grams of glucose (C6H12O6) is dissolved in 1.00 kg of water. Calculate the molality.
7. Calculate the molality when 75.0 g of MgCl2 are dissolved in 500.0 grams of solvent.
8. What is the % mass of HF if 40.0 g of HF is mixed with 500. g of water?
9. 1.5 moles of NaCl are added to 4.32 moles of H2O. What is the mole fraction of NaCl?
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Dilutions Name ____________________________ 1. Concentrated nitric acid is 15.8 M. An experiment requires 100.0 mL of 3.00 M nitric. How many ml of the concentrated are needed? 2. 150.0 ml of concentrated ammonium hydroxide, which is 14.8 M, is diluted until the final volume is 500.0 ml. What is the molarity of the final solution? 3. What volume of concentrated hydrochloric, which is 12.0 M, should be used to prepare 200.0 ml of 3.00 M acid? 4. Concentrated acetic acid is 17.4 M. How many milliliters of concentrated acetic acid would you need to prepare 1000.0 mL of 1.00 M acetic? 5. How many ml of solution would you have if you diluted 100.0 ml of 5.00 M sugar solution to a concentration of 0.75 M? 6. If I have 340 ml of a 0.5 M NaBr solution, what will the concentration be if I add 560 ml more water to it? 7. I have 400.0 mL of a 1.0 M solution. Some of the water evaporates until I have just 150.0 ml left over. What is the new concentration? 8. I needed 52 ml of concentrated hydrochloric acid solution to make 100.0 mL of 4 M acid. What was the original concentration of the acid?
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Acids and Bases Name ____________________________ Identify each substance as acid (A), base (B), conjugate acid (CA), or conjugate base (CB). 1. HC2H3O2 (aq) + H2O (l) → C2H3O2
- (aq) + H3O+ (aq) 2. OH- (aq) + HCO3
- (aq) → CO32- (aq) + H2O (l)
3. HF + H2O → H3O+ + F-
4. HCl + NH3 → Cl- + NH4
+
5. H2O + CHOOH ↔ HCOO- (aq) + H3O+ (aq)
Given the following acids, find their conjugate bases: 6. HBr __________
7. HI __________
8. H2SO4 __________
9. H2PO4 - __________
10. HCl __________
11. CH3COOH __________
12. HClO4 __________
Given the following bases, find their conjugate acids: 13. Br- __________
14. H2O __________
15. CN- __________
16. HS- __________
17. PO4-3 __________
18. NH3 __________
19. OH- __________
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Write the neutralization reaction between each acid and base. 20. Sodium hydroxide and hydrobromic acid. _______________________________________________________________________ 21. Sulfuric acid and calcium hydroxide. _______________________________________________________________________ 22. Acetic acid and lithium hydroxide. _______________________________________________________________________ 23. Ammonia and hydrofluoric acid. _______________________________________________________________________ 24. Carbonic acid and the phosphate ion (a base). _______________________________________________________________________
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Name ____________________________
Fill in the blanks accordingly.
[H+] pH pOH [OH-]
7.80
12.00
2.4 x 10-4 M
3.4 x 10-7 M
1.0 M
0.5 M
5.00
5.00
Answer the following questions and show your work. 1. Calculate the pH of a solution with 1.0 M OH- concentration. 2. If the pH of a solution is 2.37, what is the concentration of hydrogen ions? 3. What is the hydroxide ion concentration of the solution from the previous problem? 4. What is the pOH of a solution if [OH-] is 2.5 x 10-7 M? 5. What is the concentration of hydrogen ions in a solution with a pH of 5.6? 6. What is the concentration of hydroxide ions in a solution with a pOH of 9.8?
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Name ____________________________
Find the requested quantities in the following problems. You must show all of your work. 1. If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? 2. If it takes 25 mL of 0.05 M HCl to neutralize 345 mL of NaOH solution, what is the concentration of the NaOH solution? 3. If it takes 50. mL of 0.50 M KOH solution to completely neutralize 125 mL of sulfuric acid solution, what is the concentration of the H2SO4 solution? 4. Can I titrate a solution of unknown concentration with another solution of unknown concentration and get a meaningful answer? Explain your answer in a few sentences. 5. If it takes 27.4 mL of 0.768 M NaOH to titrate 16.7 mL of sulfuric acid, what is the concentration of the sulfuric acid? 6. If 24.5 mL of HCl solution is needed to titrate 33.0 mL of 0.112 M NaOH, what is the concentration of the HCl solution? 7. What is the concentration of a household ammonia cleaning solution if 49.90 mL of 0.5900 M HCl is required to neutralize 25.00 mL of solution? 8. Explain the difference between the end point and the equivalence point of a titration.
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Name ____________________________ Write the equilibrium expression for the following reactions: 1. SO3(g) + H2(g) → SO2(g) + H2O(g) 2. C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) 3. MgCO3(s) → MgO(s) + CO2(g) 4. AgCl (aq) → Ag+(aq) + Cl-(aq) 5. The reaction between nitrogen and oxygen to form NO(g) is represented by the chemical equation:
N2(g) + O2(g) → 2NO(g) The equilibrium concentrations of the gases at 1500K are 1.7x10-3M for O2, 6.4x10-3M for N2, and 1.1x10-5 M for NO. Calculate the value of Keq from these data. 6. If Keq for the reaction 2A + B → 2C is 8.0. Find the concentration of C when the concentration of A is 5.00x10-4 M and the concentration of B is 2.50 x 10-4 M.
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Name ____________________________
1. Calculate H for the reaction: C2H4 (g) + H2 (g)→ C2H6 (g), from the following data:
C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H2O (l) H= -1411. kJ
C2H6 (g) + 3 ½ O2 (g) → 2 CO2 (g) + 3 H2O (l) H= -1560. kJ
H2 (g) + ½ O2 (g) → H2O (l) H= -285.8 kJ
2. Calculate H for the reaction 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g), from the following data:
N2 (g) + O2 (g) → 2 NO (g) H= -180.5 kJ
N2 (g) + 3 H2 (g) → 2 NH3 (g) H= -91.8 kJ
2 H2 (g) + O2 (g) → 2 H2O (g) H= -483.6 kJ
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3. Calculate H for the reaction CH4 (g) + NH3 (g) → HCN (g) + 3 H2 (g), given:
N2 (g) + 3 H2 (g) → 2 NH3 (g) H= -91.8kJ
C (s) + 2 H2 (g) → CH4 (g) H= -74.9 kJ
H2 (g) + 2 C (s) + N2 (g) → 2 HCN (g) H= +270.3 kJ
4. Calculate H for the reaction 2 Al (s) + 3 Cl2 (g) → 2 AlCl3 (s), from the following data:
2 Al (s) + 6 HCl (aq) → 2 AlCl3 (aq) + 3 H2 (g) H= -1049. kJ
HCl (g) → HCl (aq) H= -74.8 kJ
H2 (g) + Cl2 (g) → 2 HCl (g) H= -1845. kJ
AlCl3 (s) → AlCl3 (aq) H= -323.kJ
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Use a standard enthalpies of formation table (below) to determine the change in enthalpy for each of these reactions.
1. NaOH(s) + HCl(g) ----> NaCl(s) + H2O(g)
2. 2 CO(g) + O2(g) ---> 2 CO2(g)
3. CH4(g) + 2 O2(g) ---> CO2(g) + 2 H2O(l)
4. 2 H2S(g) + 3 O2(g) ---> 2 H2O(l) + 2 SO2(g)
5. 2 NO(g) + O2(g) ---> 2 NO2(g)
Compound Hf (kJ/mol) Compound Hf (kJ/mol) CH4 (g) -74.8 H2S (g) -20.1 CO2 (g) -393.5 NO (g) +90.4 NaCl (s) -411.0 NO2 (g) +33.9 NaOH (s) -426.7 CO (g) -110.5 H2O (l) -285.8 SO2 (g) -296.1 H2O (g) -241.8 SO3 (g) -395.2 HCl (g) -92.3 NH3 (g) -46.2
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Equilibrium and Le Chatelier
1. Write the equilibrium expression for the following reaction: Dinitrogen pentoxide gas decomposes into nitrogen dioxide gas and oxygen gas.
2. Calculate the equilibrium constant for the reaction in problem 1 if the equilibrium concentrations are 0.50 mol/L for dinitrogen pentoxide, 0.80 mol/L for nitrogen dioxide and 0.20 mol/L for oxygen.
3. How would the equilibrium position for the equation in problem 1 be affected by: a. an addition of oxygen to the reaction vessel? b. a decrease in the pressure? c. decrease in dinitrogen pentoxide d. increase in nitrogen dioxide e. addition of a catalyst
4. Write the equilibrium constant expression for each of the following reactions:[3pts each] a. 4NO(g) + 2O2(g) 2N2O4(g) b. 2NO(g) + Br2(g) 2NOBr(g)
c. CO(g) + 2H2(g) CH3OH(g) d. SO2(g) + NO2(g) SO3(g) + NO(g)
5. What effect would an increase in pressure have on the equilibrium position of each reaction in problem 4?
6. Which value of Keq indicated most favorably for product formation and which one for reactant formation. Explain.
Keq = 1 x 1012 Keq = 1.5 Keq = 5.6 x 10-4
7. Hydrogen sulfide gas decomposes into its gaseous elements and establishes an equilibrium at 1400ºC. If a liter of this gas mixture contains 0.18 mol hydrogen sulfide and 0.014 mol hydrogen and 0.035 mol sulfur, what is the equilibrium constant for this reaction?