Free Printable Stoichiometry Multiple Choice Quiz

1.

What is Avogadro’s number?

a)

6.02 × 10²⁰

b)

6.02 × 10²³

c)

3.14 × 10²³

d)

1.00 × 10²²

2.

How many molecules are in 2 moles of CO₂?

a)

6.02 × 10²³

b)

1.20 × 10²⁴

c)

3.01 × 10²³

d)

2.00 × 10²²

3.

What is the SI unit for measuring the amount of substance in stoichiometry?

a)

Gram

b)

Mole

c)

Liter

d)

Kelvin

4.

How many atoms are in 3 moles of oxygen gas (O₂)?

a)

3.01 × 10²³

b)

6.02 × 10²³

c)

1.81 × 10²⁴

d)

3.62 × 10²⁴

5.

What is the volume of 1 mole of gas at STP?

a)

22.4 L

b)

11.2 L

c)

44.8 L

d)

2.24 L

6.

If you have 3.00 × 10²³ molecules of CO₂, how many moles do you have?

a)

0.50 moles

b)

1 mole

c)

2 moles

7.

One mole of any element contains how many atoms?

a)

1.00 x 10^20

b)

$6.02 x 10^23$

c)

$3.14 x 10^{23}$

d)

$1.00 x 10^{22}$

8.

How many moles are in $4.00 x 10^{24}$ molecules of NH3?

a)

6.64 moles

b)

8.00 moles

c)

2.00 moles

d)

0.50 moles

9.

What is the volume of 3 moles of gas at STP?

a)

11.2 L

b)

22.4 L

c)

67.2 L

d)

44.8 L

10.

If you have 0.25 moles of H2, how many molecules do you have?

a)

1.51 x 10^23

b)

3.01 x 10^23

c)

$6.02 x 10^{22}$

d)

1.00 x 10^22

11.

What is the molar mass of H2O?

a)

16 g/mol

b)

18 g/mol

c)

20 g/mol

d)

22 g/mol

12.

What is the molar mass of CO2?

a)

28 g/mol

b)

32 g/mol

c)

44 g/mol

d)

46 g/mol

13.

What is the molar mass of NaCl?

a)

58.5 g/mol

b)

60.5 g/mol

c)

35.5 g/mol

d)

22.4 g/mol

14.

What is the empirical formula of a compound containing 40% sulfur and 60% oxygen?

a)

SO

b)

SO₂

c)

S₂O

d)

S₂O₂

15.

How many atoms are in 1 mole of hydrogen gas (H₂)?

a)

6.02 × 10²³

b)

1.20 × 10²⁴

c)

3.01 × 10²³

d)

2.00 × 10²²

16.

The molar mass of Ca(OH)₂ is:

a)

56.1 g/mol

b)

74.1 g/mol

c)

100.1 g/mol

d)

44.1 g/mol

17.

Which compound has the highest molar mass?

a)

H₂O

b)

CO₂

c)

CH₄

d)

NaCl

18.

How many moles are in 90 grams of H₂O?

a)

5 moles

b)

2 moles

c)

4 moles

d)

3 moles

19.

What is the molar mass of C₆H₁₂O₆ (glucose)?

a)

120 g/mol

b)

180 g/mol

20.

What is the mass of 0.5 moles of O2 gas?

a)

16 g

b)

32 g

c)

8 g

d)

12 g

21.

What is Avogadro's number?

a)

$6.02 \times 10^{20}$

b)

$6.02 \times 10^{23}$

c)

$3.14 \times 10^{23}$

d)

$1.00 \times 10^{22}$

22.

How many moles are in 36 grams of H2O?

a)

1 mole

b)

2 moles

c)

3 moles

d)

0.5 moles

23.

Which unit is used to measure the amount of substance in stoichiometry?

a)

Grams

b)

Mole

c)

Liter

d)

Kelvin

24.

What is the molar mass of H2O?

a)

16 g/mol

b)

18 g/mol

c)

20 g/mol

d)

22 g/mol

25.

What is the volume of 1 mole of gas at STP?

a)

22.4 L

b)

11.2 L

c)

44.8 L

d)

2.24 L

26.

What is the correct mole ratio for the reaction 2H2 + O2 → 2H2O?

a)

2:2

b)

2:1

c)

1:2

d)

3:1

27.

A reaction has a theoretical yield of 120 g, but the actual yield is 90 g. What is the percent yield?

a)

75%

b)

90%

c)

125%

d)

50%

28.

How many molecules are in 2 moles of CO2?

a)

$6.02 \times 10^{23}$

b)

$1.20 \times 10^{24}$

c)

$3.01 \times 10^{23}$

d)

$2.00 \times 10^{22}$

29.

How many moles of oxygen are needed to completely react with 4 moles of CH4 in CH4 + 2O2 → CO2 + 2H2O?

a)

2 moles

b)

4 moles

c)

6 moles

d)

8 moles

30.

How many grams of NaCl can be formed from 3 moles of Na in the reaction 2Na + Cl₂ → 2NaCl?

a)

174 g

b)

58.5 g

c)

234 g

d)

97.5 g

31.

What is the empirical formula of C₆H₁₂O₆?

a)

C₆H₁₂O₆

b)

CH₂O

c)

C₂H₄O₂

d)

CHO

32.

Which law states that mass is neither created nor destroyed in a chemical reaction?

a)

Law of Conservation of Mass

b)

Boyle’s Law

c)

Charles’ Law

d)

Avogadro’s Law

33.

How many grams of CO₂ are produced when 5 moles of C₆H₁₂O₆ completely react with oxygen?

a)

180 g

b)

220 g

c)

1320 g

d)

540 g

34.

Which of the following is a limiting reactant?

a)

The reactant that is completely consumed

b)

The reactant with the highest mass

c)

The reactant that remains after the reaction

d)

The product formed in excess

35.

If 3.00 moles of H₂ react with excess N₂ according to the equation N₂ + 3H₂ → 2NH₃, how many moles of NH₃ are produced?

a)

1.00 moles

b)

2.00 moles

c)

3.00 moles

d)

6.00 moles

36.

What is the molar mass of CO₂?

a)

28 g/mol

b)

44 g/mol

c)

18 g/mol

d)

32 g/mol

37.

How many moles are in 50 grams of NaCl?

a)

0.86 moles

b)

1.23 moles

c)

2.50 moles

d)

0.50 moles

38.

What is the balanced equation for the combustion of methane?

a)

CH₄ + O₂ → CO₂ + H₂O

b)

CH₄ + 2O₂ → CO₂ + 2H₂O

c)

2CH₄ + O₂ → 2CO₂ + H₂O

d)

CH₄ + O₂ → C + H₂O

39.

What is the volume of 0.5 moles of oxygen gas at STP?

a)

11.2 L

b)

22.4 L

c)

5.6 L

d)

44.8 L

40.

If you have 112 liters of a gas at STP, how many moles of the gas do you have?

a)

2 moles

b)

5 moles

c)

10 moles

d)

4 moles

41.

If 5 moles of hydrogen gas react with nitrogen gas to produce ammonia, how many moles of ammonia are produced?

3 H $_2$ + N $_2$ --> 2 NH $_3$

a)

2.5 moles

b)

5 moles

c)

3.3 moles

d)

4.41 moles

42.

How many grams of NaCl are produced when 23 g of Na react completely with Cl $_2$ ?

(Molar mass: Na = 23 g/mol, Cl $_2$ = 71 g/mol, NaCl = 58.5 g/mol)

2 Na + Cl $_2$ --> 2 NaCl

a)

29.25 g

b)

58.5 g

c)

117 g

d)

46.5 g

43.

How many grams of $H_2O$ are produced when 2 moles of $O_2$ react completely according to the equation $2H_2 + O_2 \rightarrow 2H_2O$ ? (Molar mass of $H_2O$ = 18 g/mol)

a)

18 grams

b)

36 grams

c)

72 grams

d)

144 grams

44.

In the balanced chemical equation $N_2 + 3H_2 \rightarrow 2NH_3$ , how many moles of $H_2$ are required to react completely with 1 mole of $N_2$ ?

a)

1 mole

b)

2 moles

c)

3 moles

d)

6 moles

Stoichiometry Multiple Choice Quiz

Total questions: 44

Worksheet time: 22mins

Similar Resources on Wayground