topics covered to date: topic 1 – atoms topic 2 – formulas and equations topic 3 – chemistry...
TRANSCRIPT
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Review Book & Mid-TermTopics covered to date:
• Topic 1 – Atoms
• Topic 2 – Formulas and Equations
• Topic 3 – Chemistry Math
• Topic 4 – Matter
• Topic 5 – Periodic Table
• Topic 6 - Bonding
You must choose 4 for mid-term
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Stoichiometry
AKA Chemistry Math
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BELL RINGER
How many atoms are in a mole of carbon?
“my avogadro don't want none unless you've got moles hun”
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Ridiculous Mole Facts
3 moles of M&M’s would fill the entire earths oceans (an equivalent amount of water would fill about a ¼ cup)
1 mole of donut holes will cover the earth to a depth of seven miles!
1 mole of pennies would reach to the moon 7-8 times.
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Ridiculous Mole Facts
One mole of seconds is about 19 quadrillion years, 4,240,666 times the age of the earth, or 954,150 times the age of the universe itself.
A one liter bottle of water contains 55.5 moles of water.
If you started with a mole of pennies and spent $1,000,000 every second for 100 years, you would still have more than
99.99% of what you started with.
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Are all moles created equally?
In chemistry, how an atom reacts is dependent on the number of atoms, not the mass of the atoms.
For example, if you have 100.0 g of Na and react that with 100.0 g of Chlorine they would not react completely.
• Chlorine starts out with a mass of 35.5 and Na has a mass of 23
• As a result, we would have a bunch of Na atoms unused.
• In chemistry it is much easier to use a quantity of atoms rather than a mass of atoms
VS
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A nice mole song!
Avogadro Style
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Moles
What is the mass of a Carbon atom?
12.0 amuIf one mole of Carbon atom’s have a
mass of 12.0g, how many atoms would that be?
That would be 6.02 x 1023 atoms of carbon
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Gram Formula Mass
(molar mass)
= the mass of one mole of something
Let’s try out water: H2O
H
O
2
1
x 1.0
x 16.0
= 2.0
= 16.0
18.0 g/mol
Therefore, 1 mole of water has a mass of 18g/mol.
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GFM (practice)
Let’s try magnesium hydroxide: Mg(OH)2
Mg
O
1
2
x 24.3
x 16.0
= 24.3
= 32.0
58.3 g/mol
H 2 x 1.0 = 2.0
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GFM - Hydrates
Na2CO3●10H20Sodium Carbonate crystals:Na
C
2
1
x 23.0
x 12.0
= 46.0
= 12.0
286.0 g/mol
0 3 x 16.0 = 48.0
Hydrate - is a crystalline compound in which ions are attached to one or more WATER molecules
H20 10 x 18.0 = 180.0
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BELL RINGER
What is the gfm of NH4?
GFM = 18Moles = 72.0 ÷ 18.0 = 4 moles
“my avogadro don't want none unless you've got moles hun”
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Converting to moles
If you have 63g of water how many moles of water do you have?
1. Determine the gfm: 18 g/mol
Number of molesgiven mass (g)
gram-formula mass=
Number of moles63g
18g/mol= = 3.5 moles
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ConversionsMoles to Grams
1. How many g are in 0.0700 moles of H2O2?Number of moles
given mass (g)
gram-formula mass=
2. How many g are in 1.20 moles of CaCO3?
3 4 .0 g /m o le
xs0 .0 7 0 0 m o le
g3 8.2x
e100.1g/mol
x1.20moles
mol.120x
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GFM Practice1. NaBr
2. PbSO4
3. Ca(OH)2
4. Na3PO4
5. (NH4)2CO3
6. C6H12O6
7. Fe3(PO4)2
8. (NH4)2S
9. Zn(C2H3O2)2
10. AgF
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GFM Practice1. NaBr
2. PbSO4
3. Ca(OH)2
4. Na3PO4
5. (NH4)2CO3
6. C6H12O6
7. Fe3(PO4)2
8. (NH4)2S
9. Zn(C2H3O2)2
10. AgF
102.9 g/mol
303.3 g/mol
74.1 g/mol
164.0 g/mol
96.0 g/mol
180.0 g/mol
357.4 g/mol
68.1 g/mol
183.4 g/mol
126.9 g/mol
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BELL RINGER
You have 72.0g of NH4. How many moles do you have?
GFM = 18.0Moles = 72.0 ÷ 18.0 =
4.00 moles
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GFMWHITEBOARD REVIEW
Sodium Hydrogen Carbonate
ZincSodium CarbonateWater
SucroseC12H22O11Aluminum
Sodium ChlorideIronCopper (II)
sulfate●pentahydrate
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Some Practice1. What is the gfm for Calcium nitrate?
Number of molesgiven mass (g)
gram-formula mass=
Number of moles10.2g
164.1g/mol= = 0.0622 moles
2. How many moles of calcium nitrate do you have if you have 10.2 g?
Criss-cross to get the formula: Ca(NO3)2
Ca
N
1
2
x 40.1
x 14.0
= 40.1
= 28.0
O 6 x 16.0 = 96.0
164.1 g/mol
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Practice Problems
GFM = 122.6 g Number of moles
given mass (g)
gram-formula mass=
Number of moles40.8 g
122.6g= = 0.333 moles
1. If you have 40.8g of KClO3. How many moles do you have?
2. You have 2.5 moles of KClO3. How many grams is that? GFM = 122.6 g
Grams = GFM x # moles
Grams = 122.6g/mol x 2.5 moles = 306.5 g = 310 g
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Percent Composition
-used to find the percentage by mass of an element in a compound
What are the % of elements in dihydrogen monoxide? H2O
1 0 0% xw h o leo fm a s s
p a r to fm a s sc o m p
H 2 x 1.0 = 2.0
O 1 x 16.0 = 16.0
%= 2.0/18.0 = 11%
%= 16.0/18.0 = 88.9%
18.0 g
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Percent Composition
What are the % of elements in potassium nitrate? KNO3
1 0 0% xw h o leo fm a s s
p a r to fm a s sc o m p
K 1 x 39.1 = 39.1
O 3 x 16.0 = 48.0
% = 39.1/101.1 = 38.7%
% = 48.0/101.1 = 47.5%
101.1 g
N 1 x 14.0 = 14.0 % = 14.0/101.1 = 13.8%
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Percent Composition
What is the percentage of water in the following compound CoCl2•6H2O
Co 1 x 58.9 = 58.9
H2O 6 x 18.0 = 108.0
% = 58.9/237.9 = 24.8%
% = 108.0/237.9 = 45.40%
237.9 g/mol
Cl 2 x 35.5 = 71.0 % = 71.0/237.9 = 29.8%
Hydrate
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Percent Composition
What is the percentage of water in the following compound CaSO4•5H2OCa 1 x 40.1 = 40.1
O 4 x 16.0 = 64.0
226.2 g/mol
S 1 x 32.1 = 32.1
Hydrate
H2O 5 x 18.0 = 90.0 % = 90.0/226.2 = 39.8%
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BELL RINGER
How many grams is 0.36 moles of potassium permanganate?
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Empirical and Molecular Formulas
Empirical Formula = the formula of a compound expressed as the smallest possible whole-number ratio of subscripts of the elements in the formula
Molecular Formula = the formula of a compound in which the subscripts give the actual number of each element in the formula
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Empirical and Molecular Formulas
Molecular Formula Empirical Formula
H2O
CH3COOH
CH2OH
WO2
B2H6
C6H12O6
H2O
CH2O
CH2OH
WO2
BH3
CH2O
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Empirical and Molecular Formulas
A compound with an empirical formula of C2OH4 and a molar mass of 88 grams per mole. What is the molecular formula of the compound?
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Empirical and Molecular Formulas
A well known reagent in analytical chemistry, dimethylglyoxime, has the empirical formula C2H4NO. If its molar mass is 116.1g/mol, what is the molecular formula of the compound?
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BELL RINGER
What are the empirical formulas for the following?
C6H6
CH2ClCH3
HC2H3O2
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Determining Formulas from %Percent to massMass to molesDivide by small
Multiply ‘til whole
A compound consists of 72.2% magnesium and 27.8% nitrogen by mass. What is the empirical formula?
1. Assume 100g, so you have: 72.2g Mg and 27.8g N
2. Convert to moles
Mg - 72.2/24.3
N – 27.8/14.0
= 2.97 moles
= 1.99 moles
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Determining Formulas from %Percent to massMass to molesDivide by small
Multiply ‘til whole
3. Divide by small
Mg 2.97 / 1.99
N 1.99 / 1.99
= 1.49
= 1.00Mg1.49N1.00 ???
4. Multiply ‘til whole
Mg 1.49
N 1
X 2 = 3
X 2 = 2 Mg3N2
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Hydrate Problem• In lab, a student determined that a
hydrate of barium chloride contained 14.0% water. What is the actual numbers of water molecules for each molecule of barium chloride. Basically the formula of the hydrate.
REMEMBER
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Barium Chloride
Water 14.0%
Hydrate Problem
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BELL RINGERProblem: A compound contains 32.4% sodium, 22.1% sulfur and 45.0% oxygen. What is the empirical formula?
• Na 32.4g
• S22.1g
• O45.0g
÷ 23.0
÷ 32.1
÷ 16.0
= 1.41 mol
= 0.688 mol
= 2.81 mol
÷ .688
÷ .688
÷ .688
= 2.05
= 1.00
= 4.09
As a result the formula would be:
Na2SO4
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Hydrate PracticeA calcium chloride hydrate has a mass of 4.72 g. After heating for several minutes the mass of the
anhydrate is found to be3.56 g. Use this information to determine the
formula for the hydrate.
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Calcium Chloride
Water
Mass of Hydrate = 4.72g
Hydrate Practice (lab problem)
Anhydrous = 3.56g
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CHEMICAL REACTIONS
Reactants: Zn + I2 Product: Zn I2
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Because of the principle of the law conservation of matter,
an equation must be balanced.
It must have the same number of each kind of atoms on both sides.
Lavoisier 1788
Chemical Equations
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Chemical EquationsTheir Job: Depict the kind of
reactants and products and their relative amounts in a reaction.
Al (s) + O2 (g) ---> Al2O3 (s)
The numbers in the front are called
stoichiometric ____________coefficients
4 3 2
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• Solid (s)• Liquid (l)• Gas (g)• Aqueous solution (aq)• Catalyst H2SO4
• Escaping gas ()• Change of temperature ()
Symbols Used in Equations
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Balancing Equations
When balancing a chemical reaction you may add coefficients in front of the
compounds to balance the reaction -
but you may not change the subscripts.
Changing the subscripts changes the compound. Subscripts are determined by the valence electrons (charges for ionic
or sharing for covalent)
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Subscripts vs. Coefficients
• The subscripts tell you how many atoms of a particular element are in a compound. The coefficient tells you about the quantity, or number, of molecules of the compound.
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1. The coefficients of a chemical reaction indicate relative amounts of reactants and products.
Coefficients are MOLE RATIOS
Example: H2(g) + Cl2(g) 2HCl(g)
1 mol H2 : 1 mol Cl2 : 2 moles HCl
2. The relative masses of the reactants and products can also be determined from the coefficients.
Example:
1 mol H2 = 2.02 g H2
1 mol Cl2 = 70.90 g Cl22 mol HCl = 72.92 g HCl
Therefore, 2.02g H2 will react with 70.90g Cl2 to form 72.92g of HCl.
Why are we learning this?
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1.Compare the numbers of atoms on each side of the equation
2.Start with the most complicated molecules FIRST!
3.Leave H and O until the end4.Place COEFFICIENTS in front of the
compound to try and balance the atoms5.Check your answer to see if:
- The numbers of atoms on both sides of the equation are now balanced.
6.Reduce if possible!!!!
Steps to Balancing Equations
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___ Al(s) + ___ Br2(l) ---> ___ Al2Br6(s)2 3
Steps to Balancing Equations
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Online Balancing Equations
Click on picture above to go to the site!
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Balancing EquationsBalancing Equations
____C3H8(g) + _____ O2(g) ---->
_____CO2(g) + _____ H2O(g)
____B4H10(g) + _____ O2(g) ---->
___ B2O3(g) + _____ H2O(g)
3 4
5
2 54 10
112
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BELL RINGERBalance the following:Sodium phosphate + iron (III) oxide sodium oxide + iron (III) phosphate
Na3PO4 + Fe2O3 ----> Na2O + FePO4 2 3 2
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BELL RINGER
Balance the following:
Ca(OH)2 + H3PO4 → Ca3(PO4)2 + H2O
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• Balancing wkst
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__Al + __O2 __Al2O2
Practice Balancing Equations
2
__Fe2O3 + __H2SO4 __Fe2(SO4)3 + __H2O
__ Fe + __Cl2 __ FeCl33 22
3 3
__KClO3 → __KCl + __O22 32
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Write out the following chemical equation
Methane reacts with oxygen to produce carbon dioxide and water
CH4 + O2 CO2 + H2O
Practice
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Write out the following chemical equation
Hydrogen gas reacts in the presence of oxygen gas to explode and produce liquid water.
H2(g) + O2(g) H2O(l)
Practice
+energy
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BELL RINGER
What is the IUPAC name of the following compound?
Mn2O3
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Chemical EquationsChemical Equations4 Al(s) + 3 O2(g)
---> 2 Al2O3(s)
This equation means
4 Al atoms + 3 O2 molecules ---produces--->
2 molecules of Al2O3
AND/OR
4 moles of Al + 3 moles of O2 ---produces--->
2 moles of Al2O3
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Types of Reactions
1. Synthesis reactions
2. Decomposition reactions
3. Combustion reactions
4. Single replacement reactions
5. Double Replacement reactions• You need to be able to identify the type
of reaction and predict the product(s)
There are five types of chemical reactions we will talk about:
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1. Synthesis Reactions• Synthesis reactions occur when two
substances (generally elements) combine and form a compound. (Sometimes these are called combination or addition reactions.)
reactant + reactant 1 product• Basically: A + B AB
• Example: 2H2 + O2 2H2O
• Example: C + O2 CO2
DEMO: Write the reaction for the synthesis of MgO(s)
Mg(g) + O2(g) MgO(s)22
Zn powder + Sulfur – See Hilt
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2. Decomposition Reactions• Decomposition reactions occur when a
compound breaks up into the elements or in a few to simpler compounds
• 1 Reactant Product + Product • In general: AB A + B• Example: 2 H2O 2H2 + O2
• Example: 2 HgO 2Hg + O2
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Elephant’s Toothpase
• Write the reaction for the decomposition of hydrogen peroxide (H2O2)
H2O2 H2O + O222
Decompostion of KBrO3 – See Hilt
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Practice
• Predict the products. Then, write and balance the following decomposition reaction equations:
• Solid Lead (IV) oxide decomposes
• The formation of sulfur dioxide
PbO2(s) Pb + O2
S + O2 SO2
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3. Combustion Reactions• Combustion is actually an organic reaction• Organic Compound + O2 CO2 + H2O
• Methane Mamba
CH4 + O2 CO2 + H2O
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BELL RINGER
Write and balance the following:
Decomposition of ammonia
Formation of calcium chloride
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4. Single Replacement Reactions
• Single Replacement Reactions occur when one element replaces another in a compound.
• A metal can replace a metal (+) OR a nonmetal can replace a nonmetal (-).
• Must refer to Table J• element + compound different element + different compound
A + BC AC + B (if A is a metal) OR
A + BC BA + C (if A is a nonmetal) (remember the cation(+) always goes first!)
When H2O splits into ions, it splits into
H+ and OH- (not H+ and O-2 !!)
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Practice• Sodium chloride solid reacts with fluorine gas
NaCl(s) + F2(g) 2 2
Aluminum metal reacts with aqueous copper (II) nitrate
Al(s) + Cu(NO3)2 (aq) Cu + Al(NO3)33 232
NaF(s) + Cl2(g)
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5. Double Replacement Reactions
• Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound
• Compound + compound product + product• AB + CD AD + CB
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Double Replacement Reactions
• Mixed doubles in tennis, can the guy switch with a girl?
• Example:
AgNO3(aq) + NaCl(s) AgCl(s) + NaNO3(aq)
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Double Replacement Reactions
• Lead (II) Nitrate and Potassium Iodide
Pb(NO3)2 +
Lead (II) Iodide and Potassium Nitrate
KI PbI2 + KNO3 22
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BELL RINGER
Predict the following products and ID the reaction type:
MgCl2 + NaOH
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Practice
• Predict the product. Write and balance the following synthesis reaction equations.
Aluminum metal reacts with fluorine gas
Al(s) + F2(g) AlF33 22
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Types of Reactions Lab
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Types of Reactions LabYou need to make sure your tray has:
1 Test tube rack4 test tubesBox of matches10 ml Graduated cylinderWatch glassTest tube tongsCrucible tongsScoopulaWood splintPlastic spatulaMicrospatula
AND NO
GARBAGE!
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• Mole Calculations•
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For the Scan-Tronp. 53+54
1 – 452 – 463 – 474 – 485 – 496 – 507 – 518– 529– 5310– 5411– 5512– 5613– 57
14 – 5815 – 5916 – 6017 – 6118 – 6219 – 6320 – 6421 – 6522 – 6623 – 6724 – 6825 – 6926 – 7027 – 71
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BELL RINGER
Write and balance the following:
Magnesium and oxygen react to form magnesium oxide.
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HW Quiz
1. Decomposition of Aluminum oxide
2. Synthesis of sulfur trioxide
3. Combustion of Methane (CH4)
4. Sodium bromide and silver nitrate form sodium nitrate and silver bromide.
5. Balance the following:
C6H12O6 C2H5OH + CO2
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Lila decided to make more baked goods for the bake sale. She used 1/8
lb less flour to make bread than to make cookies. She used ¼ lb more flour to make cookies than to make
brownies. If she used ½ lb of flour to make the bread, how much flour did
she use to make the brownies?
Are you smarter than a 5th Grader ….
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StoichiometryA way to predict how many products can be made or how many reactants would be needed. You need to get the equation written correctly and balanced properly.
2H2 + O2 2H2OFor example:
You would need 2 moles of Hydrogen to make 2 moles of water
1 mole of oxygen would make 2 moles of water
If you made 6 moles of water, how much hydrogen would you need?
6 moles What would the mass of that be? 12 grams
If you had 12 moles of oxygen and 2 moles of hydrogen, how much water could you make?
2 moles of water
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StoichiometryHow many moles of gold can be liberated from the decomposition of 5.2 moles of gold (III) chloride?
2 2 3
Mass
GFM
Moles ?5.20 mol
Setup mole ratio unknowncoeff
dmoleswante
givencoeff
molesgiven
..
22
20.5 xmol molx 20.5
5.20 mol
AuCl3 Au + Cl2
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StoichiometryHow many grams of Chlorine can be liberated from the decomposition of 64.0g of gold(III) chloride?
2 2 3
Mass
GFM
Moles
?64.0g
303.5g/mol
.211 mol
Setup mole ratio unknowncoeff
dmoleswante
givencoeff
molesgiven
..
32
211. xmol molx 317.
.317 mol
71.0 g/mol
22.5 g
AuCl3 Au + Cl2
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StoichiometryHow many grams of gold can be liberated from the decomposition of 0.50 moles of gold (III) chloride?
2 2 3
Mass
GFM
Moles
?
0.50 mol
Setup mole ratio unknowncoeff
dmoleswante
givencoeff
molesgiven
..
22
50.0 xmol molx 50.0
0.50 mol
AuCl3 Au + Cl2
197.0 g/mol
98.5 g
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BELL RINGER
How many grams is 1.25 moles of Sodium hydroxide
GFM = 40Moles = 1.25 x 40 = 50 g
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BELL RINGER
Gold (III) Chloride breaks into its component elements. Write the balanced equation for this
reaction.
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BELL RINGER
Al + O2 Al2O3What is the total number of moles of O2 that must react
completely with 8.0 moles of Al in order to form Al2O3?
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StoichiometryHow many moles of carbon dioxide are needed to produce 0.333 moles of glucose in the following reaction:
CO2 + H2O C6H12O6 + O2
Don’t panic – Balance the equation
6 6 6
Mass
GFM
Moles ? 0.333 mol
Setup mole ratiounknowncoeff
dmoleswante
givencoeff
molesgiven
..
61
333. xmol molx 00.2
2.00mol
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StoichiometryWhat mass of carbon dioxide is needed to react with 54.0g of water in the following reaction:
CO2 + H2O C6H12O6 + O2
Don’t panic – Balance the equation
6 6 6
Must convert to moles – NEVER grams
Mass
GFM
Moles
? 54.0g
18.0g/mol
3.00 mol
Setup mole ratiounknowncoeff
dmoleswante
givencoeff
molesgiven
..
66
0.3 xmol
molx 0.3
3.00 mol
44.0 g/ mol
132.0 g
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BELL RINGER
KClO3(s) KCl(s) + O2(g)
If you have 20.0 g of potassium chlorate, how many moles of
oxygen could you make?
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Practice
6. KOH(aq) + CuSO4(aq)
Predict the products. Balance the equation
1. HCl(aq) + AgNO3(aq)
2. CaCl2(aq) + Na3PO4(aq)
3. Pb(NO3)2(aq) + BaCl2(aq)
4. FeCl3(aq) + NaOH(aq)
5. H2SO4(aq) + NaOH(aq)
HNO3(aq) + AgCl(s)
3 NaCl(aq) + Ca3(PO4)2(s) 62
PbCl2(s) + Ba(NO3)2(aq)
3 Fe(OH)3(s) + NaCl(aq)3
HOH + Na2SO4(aq) 2 2
K2SO4(aq) + Cu(OH)2(s) 2
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BELL RINGER
Write the balanced equation for the decomposition of potassium chlorate.
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BELL RINGER
If you wanted to make 200.0 moles of hydrogen gas from the decomposition of water, how many moles of water
would you need to start with?
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Mixed Practice
• State the type, predict the products, and balance the following reactions:
1. BaCl2 + H2SO4 2. C6H12 + O2 3. Zn + CuSO4 4. Cs + Br2 5. FeCO3
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To get Molecular Formula from Empirical Formula
Problem: You know a compound has an empirical formula of CN and a molecular mass of 52.0g. What is the molecular formula?
• Find the mass of the empirical formula
C – 12 N – 14 = 26
• How many times does that mass divide into the molecular mass?
52 / 26 = 2
C2N2
• Multiply that number to each element in the empirical formula
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Determining Formulas from %
A student starts with 25.0 g of Barium Chloride Hydrate. The student performs the lab and has 21.4 g of anhydrous salt. What was the original
formula of the hydrated crystal?
1. You already have g so you do not have to assume 100.0 g.
2. Convert to moles
Salt –
H2O –
21.4 g
Hydrated Crystals
BaCl2 208.3 g/mol
3.6 g
÷ 208.3 g/mol
÷ 18.0 g/mol
= 0.103 mol
= 0.20 mol
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Determining Formulas from %
Percent to massMass to molesDivide by small
Multiply ‘til whole
3. Divide by small
Salt
H2O
0.103 ÷ 0.103 BaCl2• ?H2O
4. Multiply ‘til whole
Do Not need to here!
Just Round
Hydrated Crystals
0.20 ÷ 0.103
= 1
= 1.94
BaCl2• 2H2O