Chapter 11 Review
Define the following:
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Stoichiometry
Mole ratio
Excess reactant
Limiting reactant
Theoretical yield
Actual yield
Percent yield
Find the following molar masses:
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O2
O
AlPO4
NaCl
C6H5Cl
CuO
Determine the number of steps for
the following problems (1, 2, or 3):
Given the following equation:
2 KClO3 –> 2 KCl + 3 O2
• How many moles of O2 can be produced
by letting 12.00 moles of KClO3 react?
• How many grams of O2 can be produced
by letting 34.7g of KClO3 react?
• How many moles of O2 can be produced
by letting 14.6g of KClO3 react?
Create the following mole ratios:
• __Ag(s) + __H2S(g) + __O2(g) __Ag2S(s) + __H2O(l)
(Equation must first be balanced.)
• Ag : H2S
• O2 : Ag2S
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Ag2S : H2O
O 2 : H 2S
Ag : O2
H2O : H2S
How many ratios can this
equation form?
What is the molar ratio of all
elements/compounds shown?
Solve the following:
Given the following equation:
2 KClO3 –> 2 KCl + 3 O2
• How many moles of O2 can be produced
by letting 12.00 moles of KClO3 react?
Solve the following:
Given the following equation:
2 KClO3 –> 2 KCl + 3 O2
• How many grams of O2 can be produced by
letting 34.7g of KClO3 react?
Solve the following:
Given the following equation:
2 KClO3 –> 2 KCl + 3 O2
• How many moles of O2 can be produced by
letting 14.6g of KClO3 react?
Solve the following:
Given the following equation:
Al2(SO3)3 + 6 NaOH  3 Na2SO3 + 2 Al(OH)3
• If 10.0 g of Al2(SO3)3 is reacted with 10.0 g of
NaOH, determine the limiting reactant
Solve the following:
Given the following equation:
2 FePO4 + 3 Na2SO4  1 Fe2(SO4)3 + 2 Na3PO4
• What is the percent yield of this reaction if takes
place with 25g of FePO4 and an excess of
Na2SO4, and produces 18.5g of Fe2(SO4)3