Free Printable Unit 4- Chemistry Test

Worksheets

Unit 4- Chemistry Test

Total questions: 55

Worksheet time: 3hrs 33mins

Name

Class

Date

Stoichiometric factors are obtained from the

balanced chemical equation

periodic table

molar mass

What are the stoichiometric factors of H₂O to H₃PO₄ in the following chemical equation? P₄O₁₀ + 6 H₂O --> 4 H₃PO₄

6/4

4/6

1/3

3/1

How many grams are in 7.8 moles of NaCl?

476grams

460 grams

452 grams

462 grams

Using the following equation:
Fe₂O₃(s) + 3H₂(g) → 2Fe(s) + 3H₂O(l)
How many moles of iron can be made from 6 moles H₂?

4 moles Fe

6 moles Fe

9 moles Fe

2 moles Fe

In the equation 2 Al₂O₃ --> 4 Al + 3 O₂, what are the stoichiometric factors of aluminum to oxygen (aluminum is asked for, oxygen is given)?

10/6

3/4

4/3

2/3

For the reaction represented by the equation $N_2+3H_{2\ }\rightarrow\ 2NH_3$ , how many moles of nitrogen (N2) are required to produce 18 grams of ammonia (NH3)?

0.9 mol

18 grams

0.53 mol

36 grams

Molar mass is in units of ________.

grams

grams/mole

mole

moles/gram

What is the mass in grams of 5.90 mol C₈H_18?

.0512 g

19.4 g

673 g

389 g

How many grams are in 11.9mol of chromium?

0.229g

4.37g

618g

619g

10.

How many moles are in 98.3 g of aluminum hydroxide Al(OH)₃?

0.794 mol

1.26 mol

2.23 mol

7.67x10³ mol

11.

2NaClO₃ (s) → 2NaCl (s) + 3O₂ (g)

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

256 g of O₂

576 g of O₂

288 g of O₂

384 g of O₂

12.

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

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

13.8 g O₂

3.91 mol of O₂

125 g O₂

41.7 g O₂

13.

Balance this reaction: ____ RbNO₃ + ____ BeF₂ ----> ____ Be(NO₃)₂ + ____ RbF

1,1,1,1

1,2,1,1

2,1,1,2

2,1,2,1

14.

What are the stoichiometric factors of H₂O to H₃PO₄ in the following chemical equation? P₄O₁₀ + 6 H₂O --> 4 H₃PO₄

6/4

4/6

1/3

3/1

15.

2 KClO₃ → 2 KCl + 3 O₂
How many moles of oxygen are produced when 6.7 moles of KClO₃ decompose completely?

6.7 mol

1.0 mol

10.1 mol

4.5 mol

16.

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.

AlCl₃

Cl₂

17.

2 KClO₃ → 2 KCl + 3 O₂
How many moles of oxygen are produced when 6.7 moles of KClO₃ decompose completely?

6.7 mol

1.0 mol

10.1 mol

4.5 mol

18.

By referring to the equation above, determine the limiting reactant if 12 moles of P₄ react with 15 moles of O_2.

P₄

P₄O₆

O₂

none of the above

19.

The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting

Percent

actual

stoichiometry

theoretical

20.

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

theoretical yield

mole ratio

actual yield

percentage yield

21.

Given the chemical equation 2Fe + 3Cl₂ --> 2FeCl₃ , how many moles of chlorine gas will be required to react with sufficient iron to produce 14 moles of iron (III) chloride?

42 mol

3 mol

21 mol

6 mol

22.

Given the equation 2CO + O₂--> 2CO₂, how many moles of CO are needed to react with 4.8 grams of O₂ gas to produce CO₂?

4 mol

0.52 mol

128 mol

0.3 mol

23.

What mass of ammonia, NH3, is necessary to react with 2.1 moles of oxygen, given 4NH₃ + 7O₂ --> 6H₂O + 4NO₂?

4.46 g

20.4 g

143 g

9.71 g

24.

The amount of product formed when a reaction is carried out in the laboratory is called?

actual yield

theoretical yield

excess yield

limiting yield

25.

The substance completely used up in a chemical reaction is called?

excess reactant

theoretical reactant

limiting reactant

actual reactant

26.

In a chemical reaction, the mass of the products:

equals the mass of reactants

is greater than the reactants

is less than the reactants

has no relationship with reactants

27.

Given 2H₂ + O₂ --> 2H₂O. How many moles of oxygen are required to react completely with 1.2 grams of hydrogen to form water?

4 mol

1.2 mol

0.5 mol

0.3 mol

28.

How many moles of CaO are produced when 68.0 g of CaCO₃ is heated according to the equation: CaCO₃ --> CaO + CO₂?

0.68 mol

0.89 mol

38 mol

68.1 mol

29.

Calculate the number of moles of water produced when 3.3 moles of Cu(NO3)2 are formed in the reaction 3Cu + 8HNO₃ --> 3Cu(NO₃)₂ + 2NO + 4H₂O.

0.3 mol

19.8 mol

2.2 mol

4.4 mol

30.

Given 2SO_2(g) + O_2(g) --> 2SO_3(g)

What is the limiting reagent when 3.1 mol of SO₂ reacts with 2.7 mol of O₂?

3.1 mol SO₂

2.7 mol O₂

31.

How many grams of Cu would be needed to react with 2.0 mol of HNO₃ in the reaction 3Cu + 8HNO₃ --> 3Cu(NO₃)₂ + 2NO + 4H₂O?

64 g

48 g

192 g

24 g

32.

Calculate the number of moles of HCl produced from 10 moles of H₂.

H₂ + Cl₂ --> 2HCl

5 mol

10 mol

2 mol

20 mol

33.

Calculate the mass of oxygen produced from the decomposition of 75.0 g of potassium chlorate. 2KClO₃ --> 2KCl + 3O₂.

19.67 g

29.5 g

112.5 g

0.922 g

34.

How many moles of carbon monoxide are needed to react with 4.80 g of oxygen gas to produce carbon dioxide? 2CO + O₂ --> 2CO₂.

0.3 mol

9.6 mol

8.4 mol

32 mol

35.

What is the molarity of a solution containing 4 moles of KCl in 2.5 L of solution?

1.6 M

0.63 M

10 M

2.6 M

36.

What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?

0.018 M

0.018 mol

1.052 M

1.052 mol

37.

What is the molarity of a solution which contains 22.41 grams of NaCl in 50.0 mL of solution?

0.488 M

7.67 mol

7.67 M

0.00767 M

38.

Molarity is measured in _____.

moles per g.

mols per L.

moles per mm.

moles per mL.

39.

What is the molarity of 2.5 mol of NaOH in 12.0 L of solution?

0.21 M

30 M

4.8 M

20.8 M

40.

Molarity is:

moles per liter of solution

written with a unit of M

calculated by dividing the moles of a substance by the liters of solvent

all of the above

41.

To convert liters of a solution to moles, one should:

divide by the molarity

multiply by the molarity

multiply by the molar mass

divide by the molar mass then multiply by the speed of light squared

42.

To convert mL to L, one should:

divide by 1000

multiply by 1000

divide by 100

multiply by 100

43.

To convert L to mL, one should:

divide by 1000

multiply by 1000

divide by 100

multiply by 100

44.

__Na + O₂ -----> __Na₂O
Type of reaction?
Balance it too. :)

Synthesis, 2Na / 4Na₂O

Decomposition, 4Na / 2Na₂O

Synthesis, 4Na / 2Na₂O

Decomposition, 2Na / 4Na₂O

45.

How many HCl molecules do you need to balance this equation?
Mg + __HCl ---> MgCl₂ + H₂

46.

Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.

1.16%

116%

85%

76%

47.

CH₄ + 2O₂ → CO₂ + 2H₂O
24 grams of CH₄ was added to the above reaction. Calculate the theoretical yield of CO₂.

66 grams

132 grams

33 grams

8.72

48.

The reaction of 25.0 g benzene, C₆H₆, with excess HNO₃ resulted in 21.4 g C₆H₅NO₂. What is the percentage yield?

C₆H₆ + HNO₃ → C₆H₅NO₂ + H₂O

100%

27.39%

54.29%

85.62%

49.

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

90.4%

104%

96.15%

1.04%

50.

What is the molar mass of sodium?

45.98

51.

What is the molar mass of fluorine gas, F₂?

18.998 g/mol

38 g/mol

9 g/mol

18 g/mol

52.

Calculate the molar mass for Al(OH)₃

78.0 g/mol

72 g/mol

28 g/mol

25 g/mol

53.

Calculate the molar mass of Cu₂O.

37 g/mol

45 g/mol

79.5 g/mol

143 g/mol

54.

Calculate the molar mass of Ba(C₂H₃O₂)₂

255.3 g/mol

237.3 g/mol

228.3 g/mol

196.3 g/mol

55.

Calculate the molar mass of KOH.

28 g/mol

56 g/mol

84 g/mol

112 g/mol

100 %

Unit 4- Chemistry Test

Total questions: 55

Worksheet time: 3hrs 33mins

Similar Resources on Wayground