WorksheetsChapter 9 Review
Total questions: 35
Worksheet time: 2hrs 2mins
Name
Class
Date
1.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
2.
Your percent yield is 80%. The actual amount of product produced was 29.1 grams. What is the theoretical yield?
a)
25.2 grams
b)
37.3 grams
c)
37.1 grams
d)
36.3 grams
3.
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%
4.
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
5.
What is the limiting reactant if 10 moles of NH3 react with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
6.
P4 + 3O2 --> P4O6
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
a)
P4
b)
O2
c)
P4O6
d)
none of the above
7.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3. If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
8.
In the equation 2 Al2O3 --> 4 Al + 3 O2, what is the mole ratio of aluminum to oxygen?
a)
10:6
b)
3:4
c)
4:3
d)
2:3
9.
How many moles of H2O are produced by 4.8 moles of O2?
2H2 +O2 -----> 2H2O
2H2 +O2 -----> 2H2O
a)
9.6 mol H2O
b)
317 mol H2O
c)
906 mol H2O
d)
3.7 mol H2O
10.
How many moles of KOH are required to make 3.0 moles of K2SO4?
H2SO4 + 2KOH -----> 2H2O + K2SO4
H2SO4 + 2KOH -----> 2H2O + K2SO4
a)
3 mol KOH
b)
6 mol KOH
c)
18 mol KOH
d)
24 mol KOH
11.
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
12.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
13.
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
14.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
15.
Which of the following do you get through measuring its mass? (No calculations)
a)
percent yield
b)
theoretical yield
c)
actual yield
d)
limiting reagent
16.
Stoichiometry is based on the law of conservation of
a)
charge
b)
mass
c)
reactants
d)
volume
17.
What is stoichiometry?
a)
The study of how the quantities of reactants and products are related in chemical reactions
b)
The study of the speed of reactions
c)
The study of how chemical reactions occur
d)
The study of types of reactions
18.
N2 + 3H2 −-> 2NH3
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
19.
N2 + 3H2 → 2NH3
How many moles of hydrogen are needed to react with 5 moles of nitrogen?
How many moles of hydrogen are needed to react with 5 moles of nitrogen?
a)
6 mol H2
b)
2 mol H2
c)
3 mol H2
d)
15 mol H2
20.
N2 + 3H2 → 2NH3
What is the mole ratio between Nitrogen and Ammonia in the above reaction?
What is the mole ratio between Nitrogen and Ammonia in the above reaction?
a)
1 moles NH3 / 2 moles N2
b)
2 moles NH3 / 1 moles N2
c)
2 moles N2 / 3 moles NH3
d)
1 moles N2 / 3 moles NH3
21.
3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe
What is the Ratio of moles of MgO to moles Fe?
What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
22.
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many grams of water can be produced from 2.3 grams of hydrogen gas?
How many grams of water can be produced from 2.3 grams of hydrogen gas?
a)
60.9 g
b)
2.04 g
c)
20.31 g
d)
4.6 g
23.
2PCl5 + 9H2O --> 10 HCl + 2H3PO4
How many moles of H2O are needed to fully react with 34.32 grams of PCl5?
How many moles of H2O are needed to fully react with 34.32 grams of PCl5?
a)
12,862.0 g
b)
208.22 g
c)
0.16 moles
d)
0.30 moles
24.
4KClO3 --> 3KClO4 + KCl
How many grams of KCl will be created when 19.2 moles of KClO3 are used up?
How many grams of KCl will be created when 19.2 moles of KClO3 are used up?
a)
5725.4 g
b)
354.84 g
c)
1431.0 g
d)
74.55 g
25.
How many grams of H2O will react with 4.5 moles of CO2?
CO2 + H2O --> H2CO3
CO2 + H2O --> H2CO3
a)
0.25 g
b)
4.00 g
c)
81.09 g
d)
15.9 g
26.
2PCl5 + 9H2O --> 10 HCl + 2H3PO4
How many grams of HCl would be produced if 54 grams of water were used?
How many grams of HCl would be produced if 54 grams of water were used?
a)
98.33g HCl
b)
31,930 g HCl
c)
48.6 g HCl
d)
1.48 g HCl
27.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
What mass of O2 will be needed to burn 36.1 g of B2H6?
What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
28.
4 Al + 3 O2 –> 2 Al2O3 How many moles of aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
29.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)
12.00 moles of NaClO3 will produce how many grams of O2?
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
30.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
31.
Calculate the molar mass of Mg(OH)2.
a)
33 g/mol
b)
41 g/mol
c)
87 g/mol
d)
58 g/mol
32.
What is the molar mass of Ba(CN)2
a)
189.37
b)
189.33
c)
189
d)
189.35
33.
What is the molar mass of Zn(C2H3O2)2
a)
392.8g/mol
b)
142.9g/mol
c)
361g/mol
d)
183.5 g/mol
34.
What is the molar mass of CH4
a)
16.05
b)
20.05
c)
10
d)
12.01
35.
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
100 %
