wayground logo

Free Printable Worksheets

NEW

Font size

S
M
L
XL
Worksheets

Chemistry Second Semester Exam Review

Total questions: 60

Worksheet time: 30mins

Name
Class
Date
1.

The chemical formula of aspirin is C9H8O4. What is the mass of 0.200 mol of aspirin?

a)

22.5 g

b)

5.4 g

c)

80 g

d)

36.0 g

2.

Which intermolecular force is the strongest?

a)

Dipole-dipole

b)

London dispersion

c)

Hydrogen bonds

3.

Which intermolecular force is the weakest?

a)

Dipole-dipole

b)

London dispersion

c)

Hydrogen bonds

4.

How many grams are in 6.50 moles of H2SO4?

a)

638 g

b)

98.1 g

c)

15.1 g

d)

0.0663 g

5.

How many particles are in 6.50 moles of H2SO4?

a)

3.91 x 1024

b)

1.08 x 10-23

c)

9.26 x 1022

d)

638

6.

If a salt dissolves in water, water serves as the

a)

Solute

b)

Solvent

c)

Solution

7.

If a salt dissolves in water, salt serves as the

a)

Solute

b)

Solvent

c)

Solution

8.

What does the triple point on a phase diagram represent?

a)

The pressure and temperature at which a liquid ceases to exist

b)

Equilibrium between the three states of matter

c)

Equilibrium between the three states of matter and six phase changes

d)

The pressure at which liquid ceases to exist

9.

What is the balanced chemical equation for the following reaction: Ba(ClO3)2 → BaCl2 + O2

a)

Ba(ClO3)2 → BaCl2 + 2 O2

b)

Ba(ClO3)2 → BaCl2 + 3 O2

c)

2 Ba(ClO3)2 → 2 BaCl2 + 3 O2

d)

2 Ba(ClO3)2 → 2 BaCl2 + 6 O2

10.

The kinetic molecular theory states that ideal gas molecules

a)

They are in constant random motion

b)

Have high densities compared with solids and liquids

c)

Exert forces of attraction and repulsion on each other

d)

Have mass and take up space

11.

In water, the following forces are present

a)

Hydrogen bonds between H and O, covalent bonds between molecules

b)

Covalent bonds between H and O, hydrogen bonding between molecules

c)

Hydrogen bonds between H and O, and between the molecules

d)

Covalent bonds between H and O, and between the molecules

12.

The following chemical equation is an example of a ___C6H6 (g) + ___O2 (g) → ___CO2 (g) + ___H2O (g)

a)

Combustion reaction

b)

Decomposition reaction

c)

Single replacement reaction

d)

Synthesis reaction

13.

If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, they are calculating the

a)

Percent yield

b)

Mole ratio

c)

Actual yield

d)

Theoretical yield

14.

What is the balanced chemical equation for the following reaction?

SF4 + H2O → SO2 + HF

a)

SF4 + 2 H2O → SO2 + 4 HF

b)

2 SF4 + 4 H2O → 2 SO2 + 8 HF

c)

SF4 + H2O → SO2 + HF

d)

3 SF4 + 6 H2O → 3 SO2 + 12 HF

15.

An aqueous solution can be defined as…

a)

A mixture of water and one or more dissolved substances

b)

A substance that is dissolved in a solvent

c)

A substance that dissolves in solutes

16.

What is the volume in liters of 0.250 mol of carbon monoxide at STP?

a)

0.112 L

b)

3.10 L

c)

5.60 L

d)

8.96 L

17.

If 525 mL of gas at 25ºC is heated to 50.ºC at a constant pressure, what would the new volume of the gas be?

a)

1050 mL

b)

569 mL

c)

263 mL

d)

484 mL

18.

A compound has the empirical formula of CH2O and a molar mass of 129.10 g/mol. What is the molecular formula of the compound?

a)

CH2O

b)

C2H4O2

c)

C5H10O5

d)

C4H8O4

19.

In what region is the substance in the liquid state only?

a)

A to B

b)

B to C

c)

C to D

d)

D to E

e)

E to F

20.

In what region is the substance in the solid state only?

a)

A to B

b)

B to C

c)

C to D

d)

D to E

e)

E to F

21.

In what region is the substance in the gas state only?

a)

A to B

b)

B to C

c)

C to D

d)

D to E

e)

E to F

22.

Where does melting occur?

a)

A to B

b)

B to C

c)

C to D

d)

D to E

e)

E to F

23.

Where does vaporization occur?

a)

A to B

b)

B to C

c)

C to D

d)

D to E

e)

E to F

24.

Where does condensation occur?

a)

B to A

b)

C to B

c)

D to C

d)

E to D

e)

F to E

25.

Where does freezing occur?

a)

B to A

b)

C to B

c)

D to C

d)

E to D

e)

F to E

26.

In what direction on the graph do endothermic and exothermic reactions occur?

a)

Endothermic: up, Exothermic: up

b)

Endothermic: up, Exothermic: down

c)

Endothermic: down, Exothermic: down

d)

Endothermic: down, Exothermic: up

27.

What is the molarity of a solution that contains 8 moles of solute in 2 L of solution?

a)

0.25 M

b)

4 M

c)

6 M

d)

8 M

28.

Name the compound PbSO4.

a)

Lead (IV) sulfate

b)

Lead (IV) disulfate

c)

Lead (II) sulfate

d)

Lead (II) disulfate

29.

In a chemical reaction, what quantities are conserved?

a)

The number of moles and the volumes

b)

The moles of reactants and moles of products

c)

The number of atoms and the mass

d)

The mass and the moles

30.

If a chemical reaction involving substance A and B stops when substance B is completely used up, substance B is referred to as the

a)

Primary reagent

b)

Limiting reagent

c)

Excess reagent

d)

Primary product

31.

The critical point on a phase diagram represents

a)

Only the temperature at which the liquid state ceases to exist

b)

Only the pressure at which the liquid state ceases to exist

c)

The temperature and pressure at which the liquid state ceases to exist

d)

The equilibrium between the three states of matter and six phase changes

32.

How many moles are in 8.5 x 1025 molecules of carbon dioxide?

a)

1.4 x 102 mol

b)

7.1 x 10-3 mol

c)

5.1 x 104 mol

d)

8.5 x 1025 mol

33.

Given the reaction: Zn (s) + 2 HCl (aq) → ZnCl2 (aq) + H2 (g). If 2.0 mol of Zn and 5.0 mol of HCl are allowed to react

a)

Zn is the limiting reagent

b)

HCl is the limiting reagent

c)

ZnCl2 is the limiting reagent

d)

H2 is the limiting reagent

34.

The following is an example of what type of chemical reaction: AB → A+B

a)

Single replacement

b)

Synthesis

c)

Decomposition

d)

Combustion

35.

The following is an example of what type of chemical reaction: AX + B → A + BX

a)

Single replacement

b)

Synthesis

c)

Decomposition

d)

Double replacement

36.

Which of the following increases the rate of solvation?

a)

An increase in temperature

b)

An increase in surface area

c)

Stirring

d)

All of these do

37.

What is the mass percent of aluminum in Al2(SO4)3?

a)

28.1%

b)

54.0%

c)

15.8%

d)

56.7%

38.

The anhydrous part of a hydrate is the

a)

Water only

b)

Salt with water

c)

Salt without water

39.

What is the molarity of a solution prepared by dissolving 1.56 g of gaseous HCl into enough water to make 26.8 mL of solution?

a)

1.59 x 104 M

b)

0.212 M

c)

1.59 M

d)

0.365 M

40.

As the temperature of a gas in a balloon decreases

a)

The volume increases

b)

The pressure increases

c)

The kinetic energy decreases

d)

All of these are true

41.

How many grams of LiNO3 are necessary to make a 1.8 m solution using 10 kg of water?

a)

18 grams

b)

1241.1 grams

c)

1000 grams

42.

When a solute is added to a solvent, it seems to fall to the bottom without dissolving. This is an example of a

a)

Unsaturated solution

b)

Saturated solution

c)

Supersaturated solution

43.

Dalton’s Law of Partial Pressure states that

a)

The total mass is equal to the sum of individual gas masses

b)

The total pressure is equal to the sum of individual gas pressures

c)

The total temperature is equal to the sum of the individual gas temperatures

44.

London dispersion forces form due to

a)

An attraction between the partially positive and negative charges of ions

b)

A temporary shift in the electrons as atoms get close to each other

c)

A permanent shift in the electrons as atoms get close to each other

d)

An attraction between H and a more electronegative atom

45.

This type of mixture has particles that can settle out if left undisturbed.

a)

Colloid

b)

Solution

c)

Suspension

d)

More than one is correct

46.

Molarity is a measure of the

a)

Concentration of moles in liters of solution

b)

Concentration of moles in kilograms of solution

c)

Concentration of grams in liters of solution

d)

Concentration of grams in kilograms of solution

47.

Molality is a measure of the

a)

Concentration of moles in liters of solution

b)

Concentration of moles in kilograms of solution

c)

Concentration of grams in liters of solution

d)

Concentration of grams in kilograms of solution

48.

What type of bond is present between a metal and a nonmetal?

a)

Covalent

b)

Ionic

c)

Metallic

49.

What type of bond is present between a nonmetal and a nonmetal?

a)

Covalent

b)

Ionic

c)

Metallic

50.

What type of bond is present between a metal and a metal?

a)

Covalent

b)

Ionic

c)

Metallic

51.

Which of the following is NOT a diatomic element?

a)

Oxygen

b)

Bromine

c)

Fluorine

d)

Helium

52.

To balance a chemical equation, you may adjust the

a)

Coefficients

b)

Subscripts

c)

Formulas of products

d)

Both coefficients and subscripts

53.

What is the percent by mass of sodium chloride solution prepared with 3.0g of NaCl and 100.0g of water?

a)

33%

b)

3.0%

c)

2.9%

d)

0.030%

54.

A solution was prepared at 50°C with 20 g of KClO3 per 100g of H2O. What type of solution was made?

a)

Unsaturated

b)

Saturated

c)

Supersaturated

55.

What compound increases in solubility the most as temperature increases?

a)

CaCl2

b)

KCl

c)

NaCl

d)

KClO3

56.

What is Boyle’s Law equation?

a)

P1V1 = P2V2

b)

V1/T1 = V2/T2

c)

(P1/T1) = (P2/T2)

d)

PV = nRT

57.

What is the Ideal Gas Law equation?

a)

P1V1 = P2V2

b)

V1/T1 = V2/T2

c)

(P1/T1) = (P2/T2)

d)

PV = nRT

58.

What is the value of the gas constant R in the Ideal Gas Law?

a)

0.0821 L atm/mol K

b)

8.314 L atm/mol K

c)

1.00 L atm/mol K

d)

22.4 L atm/mol K

59.

If 0.260 mol of Cd(C2H3O2)2 is dissolved in 0.2 kg of water, what is the molality of the solution?

a)

1 m

b)

0.8 m

c)

0.05 m

60.

If a 0.913 m solution of H2SO4 and has 1.0 kg of water, how many moles of H2SO4 are in the solution?

a)

0.91 mol

b)

1.1 mol

c)

913 mol

Similar Resources on Wayground

2nd Semester Midterm Review

65 questions

2nd Semester Midterm Review

quiz

Worksheet

•

9th - 12th Grade

Unit 1 Test Review

56 questions

Unit 1 Test Review

quiz

Worksheet

•

10th - 12th Grade

UNIT 4: Chemical Bonding & Nomenclature

55 questions

UNIT 4: Chemical Bonding & Nomenclature

quiz

Worksheet

•

10th - 12th Grade

Unit 3 Review

61 questions

Unit 3 Review

quiz

Worksheet

•

6th - 12th Grade

Atoms and Periodic Table Review

63 questions

Atoms and Periodic Table Review

quiz

Worksheet

•

10th Grade

AP Chemistry Exam Review

61 questions

AP Chemistry Exam Review

quiz

Worksheet

•

10th - 12th Grade

Using the Periodic Table

60 questions

Using the Periodic Table

quiz

Worksheet

•

9th - 10th Grade

Bonding Review

60 questions

Bonding Review

quiz

Worksheet

•

10th - 12th Grade