wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chemistry Semester 2 Review

Total questions: 73

Worksheet time: 6hrs 5mins

Name
Class
Date
1.

What does the number 3 represent in 4NH3?

a)

Subscript

b)

Superscript

c)

Coefficient

2.

What does the number 4 represent in 4NH3?

a)

Subscript

b)

Superscript

c)

Coefficient

3.

In the equation shown, what are the reactant(s)?

a)

N2 + H2

b)

NH3

4.

In the equation shown, what are the product(s)?

a)

N2 + H2

b)

NH3

5.

Is this equation balanced?

a)

Yes

b)

No

6.

Is this equation balanced?

a)

Yes

b)

No

7.

To balance an equation you should:

a)

ONLY change subscripts.

b)

ONLY change coefficients.

c)

Change BOTH subscripts and coefficients.

8.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
9.

What law governs the balancing of chemical equations?

a)

Law of Energy

b)

Law of Conservation of Matter/Mass

c)

Law of Gravity

d)

Law of Matter Movement

10.

Balance this equation

_Al +_HCl --> _H2 +_AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

11.
The following is what type of reaction:
NH3 + HCl  → NH4Cl
a)
Synthesis
b)
Decomposition
c)
Single Replacement Replacement
d)
Double Replacement Replacement
12.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
13.
What type of chemical reaction is this?
Al(OH)3 → Al2O3  + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
14.
Ions in two compounds switch. 
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
15.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
16.
Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water. 
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
17.

In a chemical reaction, 4 grams of sodium must combine with how many grams of chlorine to produce 10 grams of table salt?

a)

4 grams

b)

6 grams

c)

8 grams

d)

10 grams

18.

4 grams of hydrogen and 32 grams of oxygen will combine to form:

a)

36 grams of water

b)

28 grams of hydroxide

c)

32 grams of oxygen

d)

36 grams of deuterium

19.

Predict the products of this DR reaction: NaCl + CaO ----->

a)

Na2O + CaCl2

b)

NaCa + OCl2

c)

This reaction will not occur

d)

NaO + CaCl

20.

What are the products of this reaction: Na(NO3) + CaF2 --->

a)

This reaction will not occur

b)

NaF + Ca(NO3)2

c)

NaF2 + Ca(NO3)

d)

NaCa + F(NO3)

21.
Predict the products for the following reactants.
Mg + I2 --> 
a)
MgI
b)
MgI2
c)
Mg + I2
d)
Mg2I
22.

Predict the products for the following reactants. Na + O2 --> 

a)

NaO

b)

NaO2

c)

ONa

d)

Na2O

23.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
24.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
25.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
26.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
27.
14.5 grams of gallium (Ga) is equal to how many moles?
[1 mole Ga = 70g Ga]
a)
4.81
b)
3.22
c)
0.207
d)
0.655
28.

N2 + 3H2 --> 2NH3

What is the total number of moles of NH3 produced when 10 moles of H2 reacts completely with N2?

a)

6.7

b)

2.0

c)

3.0

d)

15.0

29.

N2 + 3H2 --> 2NH3

How many moles of N2 is needed to react with 6 moles of H2?

a)

6.7

b)

3.0

c)

2.0

d)

15.0

30.
How will the following molecule bond with itself?
a)
Dispersion
b)
Dipole
c)
Hydrogen bond
31.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
32.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
33.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
34.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
35.
London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
I2
d)
Cl2
36.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

37.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

38.

How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?

a)

83 grams

b)

75 grams

c)

40 grams

d)

12 grams

39.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
40.
When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
41.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
42.

In a solution, the part of the mixture in which other substance are dissolved

a)

Strainer

b)

Solvent

c)

Solute

d)

Magnetism

43.
Which of these solutes does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
44.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

45.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

46.

If water is a polar molecule, then which of the following must be nonpolar

a)

sugar

b)

salt

c)

oil

d)

juice

47.

Since "like dissolves like", water and oil will not mix because

a)

both of them are polar

b)

both of them are nonpolar

c)

oil is polar and water is nonpolar

d)

oil is nonpolar and water is polar

48.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
49.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

50.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
51.

If you have 34 mL of a 0.5 M NaBr solution, what will the concentration be if 56 mL of water is added to it?

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

52.

B represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

53.

A represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

54.

D represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

55.

Which component of collision theory is represented in the image?

a)

Correct orientation of molecules

b)

molecules collide with sufficient energy

c)

Products become reactants

d)

Molecules form an activated complex

56.

Is the following reaction endothermic or exothermic

a)

endothermic

b)

exothermic

57.

Is the following reaction endothermic or exothermic

a)

endothermic

b)

exothermic

58.

Which energy diagram line represents the catalyzed reaction?

a)

The black line

b)

The red line

c)

It can not be determined

59.

AgNO3 + NaCl → AgCl + NaNO3

What would you expect to happen if we decrease the temperature of this reaction container?

a)

The energy of the reactants would decrease.

b)

The would be more product produced.

c)

The number of particles of

AgNO3 and NaCl would decrease.

d)

The number of collisions in the reactants would increase.

60.

How could we make this reaction happen more quickly?

a)

Decrease the concentration of the acid

b)

crush the chalk to increase the surface area

c)

Put the test tube in an ice bath

61.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
62.

How do you calculate Enthalpy of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

63.

How much activation energy is needed for this reaction?

a)

300 KJ

b)

500 KJ

c)

400 KJ

d)

100 KJ

64.

What is the Heat of Reaction ΔH\Delta H  for this reaction?

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

65.

What is the Keq expression for this reaction?

2 NO(g)  +  O2(g) ↔  2 NO2(g)

a)

Keq = [NO2]2 / [NO]2 [O2]

b)

Keq =  [NO]2 [O2] / [NO2]2

c)

Keq = [NO]2 [O2] [NO2]2

d)

Keq = [NO2]2 / [NO]2 +  [O2]

66.

What is the correct equilibrium expression for the following reaction:

2H2O2 (aq) ↔ 2H2O (l) + O2 (g)

a)

[H2O]2[O2] / [H2O2]2

b)

[H2O2]2 / [H2O]2[O2]

c)

[O2] / [H2O2]2

d)

[H2O]2 / [H2O2]2

67.

How is the reaction quotient used to determine whether a system is at equilibrium?

a)

At equilibrium, the reaction quotient is undefined.

b)

The reaction is at equilibrium when Q < K.

c)

The reaction is at equilibrium when Q > K.

d)

The reaction is at equilibrium when Q = K.

68.

If the reaction quotient Q has a smaller value than the related equilibrium constant, K, _________

a)

the reaction is at equilibrium

b)

the reaction is not at equilibrium, and will make more products at the expense of the reactants

c)

the reaction is not at equilibrium, and will make more reactants at the expense of the products

d)

the value of K will not increase until it is equal to Q

69.

If the reaction quotient Q has a value larger than the related equilibrium constant, K _________

a)

the reaction is at equilibrium

b)

the reaction is not at equilibrium, and will make more products at the expense of reactants

c)

the reaction is not at equilibrium, and will make more reactants at the expense of products

d)

the value of K will increase until it is equal to Q

70.

Increasing the concentration of the reactants will ___.

a)

shift the reaction to the left, making more reactants

b)

shift the equilibrium to the right, making more products

c)

have no effect on the equilibrium position

d)

decrease the value of the equilibrium constant

71.

If the volume of the container is decreased at constant temperature, this will ____.

2NO2 (g) ⇌ N2O4 (g)

a)

cause a shift to the left

b)

cause a shift to the right

c)

have no effect on the equilibrium position

d)

change the value of the equilibrium constant

72.

For the reaction at equilibrium:

4H2(g) + CS2(g) ⇌ CH4(g) + 2H2S(g)

If some CH4 is removed, what will happen to the concentration of H2S in order to re-establish equilibrium?

a)

The H2S concentration will increase

b)

The H2S concentration will decrease

c)

There will be no change to the H2S concentration.

73.

Consider the reaction at equilibrium:

heat + A2(g) + 3 B2(g) ⇌ 2 AB3(g)

Which of the following stresses would cause a shift to the right?

(Select all that apply)

a)

increase the temperature

b)

decrease the temperature

c)

add more B2(g)

d)

add more AB3(g)

e)

remove some A2(g)

Similar Resources on Wayground

Honors Chem Chapter 4

72 questions

Honors Chem Chapter 4

quiz

Worksheet

•

10th Grade

Midterm Review

68 questions

Midterm Review

quiz

Worksheet

•

10th Grade

Periodic Table Test

70 questions

Periodic Table Test

quiz

Worksheet

•

9th - 12th Grade

Test 5 Test Review Spring 2022

76 questions

Test 5 Test Review Spring 2022

quiz

Worksheet

•

9th - 12th Grade

Chemistry Exam #7 Review Ionic and Covalent Bonding

69 questions

Chemistry Exam #7 Review Ionic and Covalent Bonding

quiz

Worksheet

•

10th Grade

Final Review Spring 2023

77 questions

Final Review Spring 2023

quiz

Worksheet

•

9th - 12th Grade

Exam 1 Review

76 questions

Exam 1 Review

quiz

Worksheet

•

10th - 12th Grade