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Stoich Test Review

Total questions: 81

Worksheet time: 3hrs 31mins

Name
Class
Date
1.

What is the mole-to-mole ratio for hydrogen and oxygen in the balanced equation: 2 H2 + O2 -> 2 H2O?

a)

1:2

b)

1:1

c)

3:1

d)

2:1

2.

How many moles of H2O are produced when 4 moles of O2 react? 2 H2 + O2 -> 2 H2O

a)

8 mol

b)

2 mol

c)

6 mol

d)

10 mol

3.

What is the mole-to-mole ratio between H2 and NH3 in the following balanced equation:

N2 + 3 H2 →\rightarrow 2 NH3

a)

2:3

b)

1:2

c)

1:3

d)

3:2

4.

___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

5.
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
6.

In the reaction 2H2 + O2 → 2H2O, what is the mole ratio of hydrogen to water?

a)

2 : 2

b)

2 : 1

c)

1 : 2

d)

4 : 4

7.
What is the molar mass of NaCl?
a)
58.45g/mol
b)
28g/mol
c)
12g/mol
d)
6.02 x 1023
8.
How many moles of carbon atoms are there in 5g of carbon?
a)
60 mol
b)
17 mol
c)
0.42 mol
d)
7 mol
9.
If I need 20.4 moles of sodium chloride, how much should I weigh out?
a)
0.549 g
b)
112 g
c)
1192 g
d)
5077 g
10.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
11.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
12.
Which list of number of atoms in Mg(NO2)2 is right?
a)
Mg : 1--NO :  2
b)
Mg : 1-- N :  6--O:  2
c)
Mg :  1-- N:   1--  O: 2
d)
Mg :  1-- N: 2--  O: 4
13.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
14.
What is the percent composition of Benzene, C6H6?
a)
C = 50%
H = 50%
b)
C = 85.7 %
H = 14.3%
c)
C = 92.2%
H = 7.8%
d)
C = 71.9%
H = 28.1%
15.

Molar mass of NaOH is ______________________

a)

40 grams/mol

b)

50 grams/mol

c)

45 grams/mol

d)

38 grams/nol

16.
How many moles are there in 12.7g of CaF2?
a)
0.20 mol
b)
1,000.76 mol
c)
6.14 mol
d)
0.16 mol
17.

(0901) Which conversion would you use if you need to convert from MOLES to particles?

a)

1 mole6.02 x 1023particles\frac{1\ mole}{6.02\ x\ 10^{23}particles}

b)

6.02 x 1023moles1 particle\frac{6.02\ x\ 10^{23}moles}{1\ particle}

c)

6.02 x 1023particles1 mole\frac{6.02\ x\ 10^{23}particles}{1\ mole}

d)

1 particle6.02 x 1023 moles\frac{1\ particle}{6.02\ x\ 10^{23}\ moles}

18.

(0901) Avogadro’s number is:

a)

6.02 x 1022

b)

6

c)

6.02 x 1023

d)

3.01 x 1023

19.

What is the molar mass of nitrogen gas?

a)

14

b)

28

c)

36

d)

7

20.
How many molecules of sugar (C6H12O6) are in ONE mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
21.

In order to convert Temperature to Kelvin, you add ______ to the Celsius temperature.

a)

372

b)

273

c)

237

d)

732

22.
How many moles are in 225 g of CO?
a)
28.01 mole
b)
4.82 x 1024 mole
c)
6,302,25 mole
d)
8.03 mole
23.
How many grams are in 1.2 x 1024 molecules of CO?
a)
28 grams
b)
56 grams
c)
6.02 grams
d)
1.2 grams
24.
What is the mass in grams of 6.25 mol of copper (II) nitrate?
a)
126 g
b)
785 g
c)
625 g
d)
1172 g
25.

What is the empirical formula of C4H6 ?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

26.

Which pair of molecules would have the same empirical formula?

a)

NaCrO4 and Na2Cr2O7

b)

C2H4O2 and C6H12O6

c)

C3H6O3 and C2H6O2

d)

CH4 and C2H6

27.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
28.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
29.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
 NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
30.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
31.
Whats the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of Carbon and 65.0% of oxygen?
a)
CO2Li3
b)
Li2CO3
c)
Li3CO2
d)
LiCO5
32.
A compound is a hydrate when it...
a)
is composed of only hydrogen and oxygen
b)
is a state of water
c)

contains water in the compound

d)
repels water from the compound
33.

What is the correct formula for sodium oxide?

a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
34.

What is the correct formula for Sodium Oxide Tetrahydrate?

a)

NaO * 3H2O

b)

NaO2 * 5H2O

c)

Na2O * 3H2O

d)

Na2O * 4H2O

35.

Calculate the percentage of water in :

K2CO3 · 4H2O

(a)  

36.
A hydrate of magnesium chloride is present and the following data is collected:
mass of crucible = 22.130 grams
mass of crucible + hydrate = 25.290 grams
mass of crucible and contents after heating = 23.491 grams
What is the complete formula of this hydrate?
a)
MgCl2 · 7H2O
b)
MgCl2 · 11H2O
c)
MgCl2 · 6H2O
d)
MgCl2 · 13H2O
37.
Crucible, cover: 17.8 g
Crucible, cover, and hydrate: 23.9g
Crucible, cover, and salt: 21.5g
Calculate % of water lost.
a)
90.0%
b)
60.7%
c)
39.3%
d)
45.5%
38.

Dried or without water

a)

anhydrate/anhydride

b)

hydrate

c)

grapes

39.

A 4.4 gram sample of a hydrate was heated until the water of hydration was driven off. The anhydrous compound remaining had a mass of 3.3 grams. What is the percentage by mass of water in the hydrate?

a)

75%

b)

33%

c)

67%

d)

25%

40.

Calculate the percent by mass of water in the hydrate Na2CO3 ⋅\cdot  10H2O. Be sure to round all masses from the Periodic Table to the nearest tenth and round the percent water to the correct number of significant figures. Include the correct unit with your numerical answer.

(a)  

41.

A 3.50 gram sample of a hydrate of copper sulfate yields 2.10 g of anhydrous copper (II) sulfate. Determine the mass percent of water in the hydrate.

a)

0%

b)

100%

c)

60%

d)

40%

42.
Fill in the blanks with coefficient:
PCl5+_ H2O→_ HCl+H3PO4
a)
4, 5
b)
1, 6
c)
3, 8
d)
2,2
43.
The blue numbers in the image below represent ________
a)
Charges
b)
coefficients
c)
subscripts
d)
none of the answers are correct
44.
Balance this equation:
P4+O2  -->  P2O3
a)
3 P4+ O2 --> 2 P2O3
b)
 P4+ O2 --> 2 P2O3
c)
 P4+ 3 O2 --> 2 P2O3
d)
 P4+ 2 O2 --> 3 P2O3
45.
N2 + H2 = NH4
a)
Balanced
b)
Unbalanced
46.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
47.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number in front of a chemical formula.
c)
The number in between the chemical symbols.
d)
The number behind a chemical formula.
48.
What is the part of the chemical equation in green called? 
Fe + S --> FeS
a)
products
b)
reactants
c)
yield
d)
chemical formula
49.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
50.

Identify the following chemical reaction.

Pb + FeSO4 ----> PbSO4 + Fe

a)

Synthesis (or combination)

b)

Decomposition

c)

Single displacement

d)

Double displacement

51.

Identify the following chemical reaction.

3 HBr + 1 Al(OH)3 ----> 3 H­2O + 1 AlBr3

a)

Synthesis (or combination)

b)

Decomposition

c)

Single displacement

d)

Double displacement

52.

What reaction has the following general formula:

AB --> A + B

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

53.

What is the right part of a chemical equation called?

2H2 + O2 ---> 2H2O

a)

Reactants

b)

Products

c)

Coefficients

d)

Subscripts

54.

Of the reactions below, which one is not a synthesis reaction?

a)

C + O2 --> CO2

b)

2N2 + 3H2 --> 2NH3

c)

2CH4 + 4O2 --> 2CO2 + 4H2O

d)

2Mg + O2 --> 2MgO

55.

What type of reaction is this?

3KOH + H3PO4 --> K3PO4 + 3H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

56.

Which of the following equations are correctly balanced?

a)

12CO2 + H2O ---> C6H12O6 + O2

b)

CO2 + 9H2O ---> C6H12O6 + O2

c)

CO2 + H2O ---> 3C6H12O6 + O2

d)

6CO2 + 6H2O ---> C6H12O6 + 6O2

57.

What type of reaction is this? 2 Pb(NO3)2 --> 2 PbO + 4 NO2 + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

58.
___C3H8 +___O2 --> ___CO2 + ___H2O
a)
1,5,3,4
b)
2,10,6,8
c)
already balanced
d)
1,5,5,4
59.
__Al + __Fe3N2 -->__AlN + __Fe
a)
already balanced
b)
4,2,4,6
c)
2,1,2,3
d)
1,2,1,3
60.
Which chemical reaction breaks down into 2 substances?
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
61.
Identify this type of reaction,
Cl2 + 2KI -->  I2 + 2KCl
a)
Synthesis
b)
Single Replacement
c)
Double Replacement
d)
Decomposition
62.

What is the molecular formula of a compound with an empirical formula of CH2O and a molar mass of 180 g/mol?

a)

C2H4O2

b)

C4H8O4

c)

C6H12O6

d)

C3H6O3

63.

Which of the following is a balanced chemical equation?

a)

2H2 + 2O2 → 2H2O

b)

H2 + O2 → H2O

c)

H2 + 2O2 → H2O2

d)

2H2 + O2 → 2H2O

64.

What is the percent composition of oxygen in H2O?

a)

44.4%

b)

88.8%

c)

33.3%

d)

11.2%

65.

What is the empirical formula of a compound that contains 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass?

a)

CHO

b)

C3H6O3

c)

C2H4O2

d)

CH2O

66.

Which of the following is a double displacement reaction?

a)

NaCl + AgNO3 -> NaNO3 + AgCl

b)

Fe + CuSO4 -> FeSO4 + Cu

c)

H2 + O2 -> H2O

d)

C + O2 -> CO2

67.

What is the molar mass of sulfuric acid (H2SO4)?

a)

100 g/mol

b)

98 g/mol

c)

102 g/mol

d)

96 g/mol

68.

What is the empirical formula of a compound that contains 40% sulfur and 60% oxygen by mass?

a)

S2O4

b)

S2O3

c)

SO2

d)

SO

69.

Balance the following chemical equation:
C3H8 + O2 → CO2 + H2O

a)

C3H8 + 6O2 → 3CO2 + 4H2O

b)

C3H8 + 4O2 → 3CO2 + 4H2O

c)

C3H8 + 5O2 → 2CO2 + 4H2O

d)

C3H8 + 5O2 → 3CO2 + 4H2O

70.

What is the molar mass of H2SO4?

a)

96.07 g/mol

b)

100.10 g/mol

c)

98.08 g/mol

d)

102.09 g/mol

71.

In the complete reaction of 22.99 g of sodium with 35.45 g of chloride, what mass of sodium chloride is formed?

(a)  

72.

A 10.0 g sample of magnesium reacts with oxygen to form 16.6 g of magnesium oxide.  How many grams of oxygen reacted?

(a)  

73.
If reaction starts with 20g of reactants it should produce 
a)
a total of 40g of products
b)
a total of 10g of products
c)
a total of 80 g of products
d)
a total of 20g of products
74.

A student heated a 10 gram sample of a chemical in an open container. A chemical reaction occurred, and the mass of the sample was measured again. The mass of the sample was found to be less than before the reaction. Which of the following best explains the decrease in mass of the sample?

a)

The heat caused the chemical to become less dense.

b)

The reaction gave off more heat than was added.

c)

Some of the lighter particles were destroyed.

d)

Some of the particles escaped as a gas formed.

75.
Jamie weighs a glass of water and observes its weight to be 12 ounces. Jamie then adds 6 ice cubes to the glass of water. Each ice cube weighs one ounce. After all of the ice cubes have melted, what will be theapproximate weight of the glass of water?
a)
6 
b)
12 
c)
18 ounces
76.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
77.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 
a)
Warm
b)
Cold
78.

According to the law of conservation of mass, how much mercury was present in the mercury (II) oxide?

a)

55.8 g

b)

64.2 g

c)

60.0 g

d)

126.0 g

79.

What is the empirical formula of a compound that contains 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass?

a)

CH3O

b)

C2H4O2

c)

CH2O

d)

C3H6O3

80.

How many grams of water are produced when 5 moles of hydrogen gas react with excess oxygen gas? 2 H2 + O2 -> 2 H2O

a)

90 g

b)

36 g

c)

180 g

d)

45 g

81.

What is the molar mass of calcium carbonate (CaCO3)?

a)

50 g/mol

b)

200 g/mol

c)

150 g/mol

d)

100 g/mol

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