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STOICHIOMETRY

Total questions: 30

Worksheet time: 2hrs 38mins

Name
Class
Date
1.

2NaClO3 (s) → 2NaCl (s) + 3O2 (g)

12.00 moles of NaClO3 will produce how many grams of O2?

NaClO3 = 106.44 g/mol ; O2 = 32.00 g/mol

a)

256 g of O2

b)

576 g of O2

c)

288 g of O2

d)

384 g of O2

2.

From the reaction: B2H6 + 3O2 -->2 HBO2 + 2 H2O

What mass of O2 will be needed to burn 36.1 g of B2H6?

B2H6 = 27.68 g/mol

a)

13.8 g O2

b)

3.91 mol of O2

c)

125 g O2

d)

41.7 g O2

3.

18.26 mL of a 1.50 mol/L hydrochloric acid reacts with magnesium hydroxide. Calculate the mass of magnesium hydroxide needed for the reaction.

Mg(OH)2 + 2 HCl -> 2 H2O + MgCl2

Mg(OH)2 = 58.33 g/mol ; HCl = 36.46 g/mol

a)

4.68 g Mg(OH)2

b)

0.799 g Mg(OH)2

c)

0.0274 Mg(OH)2

d)

1.60 g Mg(OH)2

4.
Balance this reaction: ____ RbNO3 + ____ BeF2 ----> ____ Be(NO3)2 + ____ RbF
a)
1,1,1,1
b)
1,2,1,1
c)
2,1,1,2
d)
2,1,2,1
5.
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
6.

What is the percent yield of the following reaction if 145g of P2O5 reacts with 40 grams of water, but you only collected 112 grams of phosphoric acid (MW 98g/mol)?  3 H2O + P2O5 -> 2H3PO4

a)
80%
b)
85%
c)
77%
d)
58%
7.

For the reaction represented by the equation Cl2 + 2KBr → Br2 + 2KCl, how many grams of potassium chloride can be produced from 356 grams potassium bromide? (atomic masses: K=39 Cl=35.5 Br=80)

a)
749 g
b)

223 g

c)
479 g
d)
814 g
8.

2Al + 3H2SO4 -> Al2(SO4)3 + 3H2 How many grams of aluminum sulfate (MW 342g/mol) would be formed if 250g H2SO4 (MW 98g/mol) completely reacted with aluminum?

a)
0.85 g
b)

291 g

c)
450 g
d)
870 g
9.

Use the following equation: 2NaOH(aq) + H2SO4(aq) --> 2H2O(l) + Na2SO4(aq) How many grams of sodium sulfate (MW 142g/mol) will be formed if you start with 200 grams of sodium hydroxide (MW 40g/mol) ?

a)

150 g Na2SO4

b)

593 g Na2SO4

c)

330 g Na2SO4

d)

355 g Na2SO4

10.

___KNO3 → ___KNO2 + ___O2

What coefficients are needed to balance the reaction?

a)

2, 2, 1

b)

2, 3, 2

c)

1, 2, 2

d)

1, 3, 1

11.

In the equation 6CO2+6H2O → C6H12O6+6O26CO_2+6H_2O\ \rightarrow\ C_6H_{12}O_6+6O_2  the mole ratio of water to oxygen is:

a)

2 : 1

b)

1 : 1

c)

3 : 2

d)

6 : 8

12.

In the equation Al2(SO4)3+3Ca(OH)2 → 3CaSO4 +2Al(OH)3Al_2\left(SO_4\right)3+3Ca\left(OH\right)_2\ \rightarrow\ 3CaSO_4\ +2Al\left(OH\right)_3  , , the mole ratio of calcium hydroxide to aluminum hydroxide is:

a)

1 : 3

b)

2 : 3

c)

1 : 1

d)

3 : 2

13.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
14.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
15.

              For the reaction represented by the equation N2+3H2 → 2NH3N_2+3H_{2\ }\rightarrow\ 2NH_3  , how many moles of nitrogen (N2) are required to produce 18 grams of ammonia (NH3)?

a)

0.9 mol

b)

18 grams

c)

0.53 mol

d)

36 grams

16.
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
17.

In the reaction represented by the equation CH4(g) + O2(g) ----> CO2(g) + H2O(g), a mass of 125 g CH4is reacted with excess oxygen. The expression:

125 g CH4 ×1 mol CH416.05 g CH4×2 mol H2O 1 mol CH4×18.20 g H2O1 mol H2O125\ g\ CH_{4\ }\times\frac{1\ mol\ CH_4}{16.05\ g\ CH_4}\times\frac{2\ mol\ H_2O\ }{1\ mol\ CH_4}\times\frac{18.20\ g\ H_2O}{1\ mol\ H_2O}  

is used to calculate the:

a)

mass of oxygen redacted.

b)

mass of carbon dioxide produced.

c)

mass of water produced.

d)

none of the above.

18.

What is the mole ratio of H2O to H3PO4 in the following chemical equation?

P4O10+6H2O → 4H3PO4P_4O_{10}+6H_2O\ \rightarrow\ 4H_3PO_4  

a)

1 to 6

b)

3 to 2

c)

4 to 6

d)

2 to 3

19.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
20.
What is a Limiting Reagent?
a)
speeds up a reaction
b)
what you run out of first
c)
what you have left over
d)
slows down a reaction
21.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
22.
True or False. You must convert grams to moles to do stoichiometry.
a)
True
b)
False
23.
KNO3 --> KNO2 + O2
What coefficients are needed to balance the reaction?
a)
2, 2, 1
b)
2, 3, 2
c)
1, 2, 2
d)
1, 3, 1
24.
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
25.
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
26.

How many liters of Fe2(SO4)3 can be produced if you start with 2.5 moles H2SO4?

3 H2SO4 + 2 Fe >> Fe2(SO4)3 + 3 H2

a)

2.5 L

b)

22.4 L

c)

168 L

d)

18.7 L

27.

If 30 liters of hydrogen gas (H2) are produced, how many liters of oxygen gas (O2) would be produced?

2H2O >> 2H2 + O2

a)

30 L

b)

60 L

c)

15 L

d)

22.4 L

28.

How many grams of KCl are produced if 25 g of KClO3 decompose?

2 KClO3 >> 2 KCl + 3 O2

a)

15.2 g

b)

40.8 g

c)

18.75 g

d)

2.0 g

29.

If 55.4 g of Fe2O3 reacts with an excess of CO, Fe is produced. What is the theoretical yield of iron?

Fe2O3 + 3 CO >> 2 Fe + 3 CO2

a)

43.2 g

b)

160 g

c)

59.4 g

d)

38.8 g

30.

From the reaction: B2H6 + 3O2 -->2 HBO2 + 2 H2O

What mass of O2 will be needed to burn 36.1 g of B2H6?

B2H6 = 27.68 g/mol

a)

13.8 g O2

b)

3.91 mol of O2

c)

125 g O2

d)

41.7 g O2

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