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stoichiometry practice

Total questions: 75

Worksheet time: 5hrs 32mins

Name
Class
Date
1.
State whether the following compound is soluble or insoluble.  calcium carbonate CaCO3 
a)
soluble
b)
insoluble
2.
State whether the following compound is soluble or insoluble. potassiun bromide KBr
a)
Soluble
b)
Insoluble
3.

Which of the following best describes a precipitate?

a)

solid powder that falls out of solution when a solid and liquid reactant combine

b)

solid powder that falls out of solution when two aqueous reactants combine

c)

solid powder that falls out of solution when aqueous and gaseous reactants combine

4.

NH4Br

a)

Soluble

b)

Insoluble

5.

Will this compound dissolve in water?

MgCl2

a)

Yes, it will dissolve.

b)

No, it will not dissolve.

6.
K2CO3
a)
soluble
b)
insoluble
7.

Al2S3

a)

Soluble

b)

Insoluble

8.

Which of the following compounds is SOLUBLE?

a)

copper carbonate

b)

calcium carbonate

c)

potassium carbonate

d)

strontium carbonate

9.
State whether the following compound is soluble or insoluble. Zinc hydroxide Zn(OH)2
a)
Soluble 
b)
Insoluble
10.

Na2CO3

a)

Soluble

b)

Insoluble

11.

Will this compound dissolve in water?

AgCl

a)

Yes, it will dissolve.

b)

No, it will not dissolve.

12.

Will this compound dissolve in water?

Ag(ClO4)

a)

Yes, it will dissolve.

b)

No, it will not dissolve.

13.
Silver acetate
a)
Soluble 
b)
Insoluble
14.
KOH
a)
Soluble 
b)
Insoluble
15.

Solubility Rule 1 does NOT apply to which of these compounds?

a)

LiOH

b)

Mg(NO3)2

c)

Fe(CH3COO)3

d)

BaSO4

16.

CaSO4 is insoluble (s) based on which rule on the solubility chart?

a)

Rule 1

b)

Rule 2

c)

Rule 4

d)

Rule 7

17.

BaCO3 is insoluble (s) based on which rule on the solubility chart?

a)

Rule 1

b)

Rule 2

c)

Rule 5

d)

Rule 6

18.

NaOH is soluble (aq) based on which rule on the solubility chart?

a)

Rule 1

b)

Rule 3

c)

Rule 4

d)

Rule 6

19.

NiF2 is soluble (aq) based on which rule on the solubility chart?

a)

Rule 1

b)

Rule 2

c)

Rule 3

d)

Rule 4

20.

Ca(NO3)2 is soluble (aq) based on which rule on the solubility chart?

a)

Rule 1

b)

Rule 2

c)

Rule 5

d)

Rule 7

21.
Zinc Carbonate
a)
Soluble 
b)
Insoluble 
22.
Silver Iodide
a)
Soluble 
b)
Insoluble 
23.
Zinc Hydroxide
a)
Soluble 
b)
Insoluble
24.
KBr
a)
Soluble
b)
Insoluble
25.
State whether the following compound is soluble or insoluble.  calcium carbonate CaCO3 
a)
soluble
b)
insoluble
26.

Which of the following is not a strong base?

a)

Ca(OH)2

b)

KOH

c)

NH3

d)

LiOH

e)

Sr(OH)2

27.

How many grams of Ag2CrO4 will precipitate when 150 mL of 0.500 M solution of AgNO3 are added to excess amount of K2CrO4?

2 AgNO3 + K2CrO4 --> Ag2CrO4 + 2 KNO3

a)

12.4 g

b)

39.1 g

c)

56.4 g

d)

72.9 g

28.

Suppose you have 500 mL of a 2.5 M solution of H3PO4 and excess magnesium hydroxide. How many grams of magnesium phosphate (Mg3(PO4)2 would form?

3 Mg(OH)2 + 2 H3PO4 --> Mg3(PO4)2 + 6 H2O

a)

324 g

b)

1.25 g

c)

164 g

d)

2.03 g

29.

An aliquot of KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What mass of KOH was in the original sample?

KOH + HCl --> KCl + H2O

a)

1.6 g

b)

0.17 g

c)

0.21 g

d)

7.2 g

30.

Starting with 150.0 mL of 2.50 M solution of Na3PO4 how many moles of Ca3(PO4)2 will precipitate?

3 CaCl2 + 2 Na3PO4 --> Ca3(PO4)2 + 6 NaCl

a)

0.375 mol

b)

0.750 mol

c)

0.075 mol

d)

0.188 mol

31.

How many mL of 0.5M HNO3 would be needed to react with 85mL of 0.75M KOH?

a)

127.5mL

b)

0.1275mL

c)

31.9mL

d)

0.031875mL

32.
What mass in (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of aqueous hydrobromic acid?
a)
53.6
b)
1.44
c)
1.23
d)
34.5
33.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
34.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

35.

Solutions of acetic acid and sodium bicarbonate react to form sodium acetate, water and carbon dioxide gas:

HC2H3O2 (aq) + NaHCO3(aq) --> NaC2H3O2 (aq) + H2O (l) CO2 (g) What mass of water will be formed if 145.0 mL of 1.5 M acetic acid is mixed with 195.0 mL of 1.25 M sodium bicarbonate solution? (Note: this is a limiting reactant problem—use a BCA table)

a)

6.7 g

b)

2.5 g

c)

3.9 g

d)

1.6 g

e)

10.4 g

36.

Lithium metal reacts with phosphoric acid to form hydrogen gas in the following (dangerous) reaction:

6 Li (s) + 2 H3PO4 (aq) --> 3 H2 (g) + 2 Li3PO4 (aq) What volume of 2.30 M phosphoric acid will be needed to form 19.7 L of hydrogen gas at STP? (Remember: 1 mole of any gas at STP is 22.4 L)

a)

466 mL

b)

255 mL

c)

133 mL

d)

322 mL

e)

75 mL

37.

Solid iron (II) sulfide reacts with hydrochloric acid to form hydrogen sulfide gas and aqueous iron (II) chloride:

FeS (s) + 2 HCl (aq) --> H2S (g) + FeCl2 (aq) If 145 mL of HCl is needed to completely react with 25 g of iron (II) sulfide, what is the concentration of the HCl solution?

a)

3.1 M

b)

0.68 M

c)

2.7 M

d)

9.0M

e)

3.9 M

38.

Aqueous solutions of sodium chloride and lead (II) nitrate react to form solid lead(II) chloride in the following balanced equation: 2 NaCl (aq) + Pb(NO3)2 (aq) --> PbCl2 (s) + 2 NaNO3 (aq) What is the theoretical yield of lead(II) chloride if 250.0 mL of 1.75 M sodium chloride reacts with excess lead(II) nitrate?

a)

78.5 g

b)

93.1 g

c)

45.5 g

d)

60.8 g

e)

59.4 g

39.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
40.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
41.

18.26 mL of a 1.50M hydrochloric acid reacts with excess magnesium hydroxide. Calculate the mass of magnesium hydroxide needed for the reaction.

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

a)

4.68 g Mg(OH)2

b)

0.798 g Mg(OH)2

c)

0.0274 Mg(OH)2

d)

1.07 g Mg(OH)2

42.

FeS (s) + 2 HCl (aq) --> H2S (g) + FeCl2 (aq)

If 145 mL of HCl is needed to completely react with 25 g of iron (II) sulfide, what is the concentration of the HCl solution?

a)

3.1 M

b)

0.68 M

c)

2.7 M

d)

9.0M

e)

3.9 M

43.

CaCO3 + 2 HCl --> CaCl2 + H2O + CO2

What volume (in mL) of 1.35 M HCl will be needed to completely react with 3.82 g of solid CaCO3?

a)

56.5 mL

b)

47.2 mL

c)

61.6 mL

d)

34.7 mL

e)

124 mL

44.

How many mL of 0.5M HNO3 would be needed to react with 85mL of 0.75M KOH?

a)

127.5mL

b)

0.1275mL

c)

31.9mL

d)

0.031875mL

45.

What mass of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of aqueous hydrobromic acid?

AgNO3 + HBr --> HNO3 + AgBr

a)

53.6

b)

1.44

c)

1.23

d)

34.5

46.
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%
47.
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
48.
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
49.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
50.
a)

True

b)

False

51.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

52.
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%
53.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
54.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

55.

Cl2 + 2KBr → Br2 + 2KCl

How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?

a)

749 g

b)

223 g

c)

479 g

d)

814 g

56.

If a chemist calculates the maximum amount of product that could be obtained from a chemical reaction, he or she is calculating the

a)

Theoretical yield

b)

Mole ratio

c)

Actual yield

d)

Percentage yield

57.
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 (KBr)?
a)
749 g
b)
225 g
c)
479 g
d)
814 g
58.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
59.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 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
60.
Use the following equation:
NaIO3(aq) + 6HI(aq) --> 3I2(s) + NaI(aq) + 3H2O(l)
How many moles of iodine can be made from 6.55 moles of NaIO3?
a)
4.55 moles I2
b)
23.18 moles I2
c)
19.65 moles I2
d)
34.99 moles I2
61.
 CaC₂(s) + 2H₂O(l)   -->   C₂H₂(g)   + Ca(OH)₂(aq)
how many grams of Ca(OH)₂ would be formed with 3.20 moles of CaC₂?
a)
119 g
b)
21.2 g
c)
114 g
d)
237 g
62.
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
63.
4 Al + 3 O2 –> 2 Al2O3  How much 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
64.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
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
65.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
66.
When reacting Na with Cl2, we calculated that the theoretical yield should be 12.5 grams. Our actual yield was 13.0 grams. What is the percent yield?
a)
100%
b)
104%
c)
96%
d)
1.04
67.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)

6 mol H

b)

2 mol H

c)

3 mol H

d)

1 mol H

68.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
69.
What is the molar mass of C6H12O6?
a)

180.18 g/mol

b)

180.12 g/mol

c)

180.24 g/mol

d)

180.06 g/mol

70.
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
71.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
72.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of Al2(SO4)3 would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
73.

B2H6 + 3O2 -->2 HBO2 + 2 H2O  

How many grams 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
74.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
75.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many grams of HCl are consumed by the reaction of 2.50 moles of magnesium?
a)
5.00 g
b)
7.29
c)
182 g
d)
218 g

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