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WorksheetsCompound Stoichiometry
Total questions: 25
Worksheet time: 2hrs 49mins
Name
Class
Date
1.
What is the molar mass of CH4
a)
16.0
b)
16.4
c)
16.03
d)
13
2.
2H2 + O2 −−〉 2H2O
8.3 moles H2 −−〉moles H2O
8.3 moles H2 −−〉moles H2O
a)
4.15
b)
8.3
c)
16.6
d)
74.04
3.
2H2 + O2 −−〉 2H2O
3.91 g O2 −−〉g H2O
3.91 g O2 −−〉g H2O
a)
1.905
b)
4.4
c)
2.2
d)
1.1
4.
Find the percent yield
2Fe2O3 + 3C −−〉 4Fe + 3CO2
Given 38.1 grams iron(III) oxide and 9.53 grams of carbon, find the percent yield if the actual yield is 17.41 grams of iron.
2Fe2O3 + 3C −−〉 4Fe + 3CO2
Given 38.1 grams iron(III) oxide and 9.53 grams of carbon, find the percent yield if the actual yield is 17.41 grams of iron.
a)
65.3
b)
29.4
c)
26.65
d)
59.14
5.
What is the molar mass of Ba(CN)2
a)
189.3
b)
189.0
c)
189
d)
189.4
6.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant? C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
7.
In a lab, a scientist calculates he should produce 12.3 grams of product in his experiment. When he is finished collecting his product, it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
8.
Molar masses are determined from
a)
the mole ratio of a given amount of reactant to an unknown amount of product
b)
the periodic table
c)
any mole ratio in the equation
d)
a conversion factor
9.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
53.985 g
d)
14 g
10.
Actual yield must be determined by
a)
experiments
b)
calculations
c)
theoretical yield
d)
estimation
11.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
12.
What is the theoretical yield?
a)
the maximum amount of product from a reaction
b)
the amount of product recovered from a lab experiment
c)
amount of product that causes the reaction to stop
d)
the amount of product needed to reverse the reaction
13.
Using the balanced equation,
Mg(s) + 2 HCl(aq) --> MgCl₂(aq) + H₂(g)
How many moles of HCl are consumed in the production of 7.5 moles of MgCl₂?
Mg(s) + 2 HCl(aq) --> MgCl₂(aq) + H₂(g)
How many moles of HCl are consumed in the production of 7.5 moles of MgCl₂?
a)
3.8 moles
b)
15 moles
c)
7.5 moles
d)
23 moles
14.
Which compound has the smallest molar mass?
a)
CO
b)
CO2
c)
H2O
d)
H2O2
15.
N2 + 3H2 −-> 2NH3
How many moles of ammonium are produced when 3 moles of nitrogen react with hydrogen?
How many moles of ammonium are produced when 3 moles of nitrogen react with hydrogen?
a)
6 moles Ammonium
b)
1.5 moles ammonium
c)
9 moles ammonium
d)
9 moles hydrogen
16.
Find the percent yield
2Fe2O3 + 3C −−〉 4Fe + 3CO2
38.1 g Fe2O3 −−〉 Fe
9.53 g C −−〉 Fe
Actual yield = 17.41
2Fe2O3 + 3C −−〉 4Fe + 3CO2
38.1 g Fe2O3 −−〉 Fe
9.53 g C −−〉 Fe
Actual yield = 17.41
a)
65.3
b)
29.4
c)
26.65
d)
59.14
17.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
18.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
19.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant? C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
20.
Calculate the molar mass of Mg(OH)2.
a)
33.2 g/mol
b)
41.3 g/mol
c)
86.9 g/mol
d)
58.3 g/mol
21.
Stoichiometry is based on the law of conservation of
a)
charge
b)
mass
c)
reactants
d)
volume
22.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
23.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
24.
How many atoms are in 1 mole of CO2?
a)
4.6 atoms
b)
4.6 grams
c)
6.02 x 10 ^23 atoms
d)
.036 atoms
25.
What is the molar mass of C6H12O6?
a)
180.18
b)
180.12
c)
180.24
d)
180.06
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