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Chemistry Second Semester Review (2026)

Total questions: 57

Worksheet time: 1hrs 8mins

Name
Class
Date
1.

Which reactant controls the amount of product formed in a chemical reaction?

a)

Limiting reactant (reagent)

b)

Excess reactant (reagent)

c)

First reactant (reagent)

d)

Extra reactant (reagent)

2.

____ deals with the mass relationships of elements in compounds and the mass relationships among reactants and products in chemical reactions.

a)

Molar mass

b)

Stoichiometry

c)

Avagadro's number

d)

Molar volume

3.

The maximum amount of product calculated to be obtained in a chemical reaction is the _____________

a)

Actual yield

b)

Theoretical yield

c)

Percent yield

d)

Product

4.

In the following equation what is the mole ratio of chlorine to hydrogen chloride?

H2 + Cl2 --> 2HCl

a)

1:1

b)

2:1

c)

2:2

d)

1:2

5.
What are the 2 characteristics of matter?
a)
volume & energy
b)
mass & energy
c)
volume & mass
d)
matter encompasses all
6.
The amount of space an object takes up. 
a)
volume
b)
mass
c)
matter
d)
energy
7.
Gas has mass & takes up space.
a)
true 
b)
 false
8.
Which state of matter has indefinite shape & volume?
a)
solid 
b)
liquid 
c)
gas
9.
True or false. Heat travels from an area lower concentration (object with less heat) to an area of higher concentration (object with more heat). Hint: Think about the heat transfer between ice & water in a glass.
a)
True
b)
False
10.
Which state of matter has the highest kinetic energy (atoms move the fastest)?
a)
solid
b)
liquid 
c)
gas
11.
In which state of matter are the atoms spaced the closest together?
a)
solid
b)
liquid
c)
gas
12.
In which state of matter are the atoms spaced the farthest apart & are the most compressible?
a)
solid 
b)
liquid
c)
gas
13.
Dry ice is an example of what phase change.
a)
freezing
b)
melting
c)
vaporization/boiling
d)
sublimation
14.
When ice melts does kinetic energy decrease (release heat) or increase (absorb heat)?
a)
kinetic energy decreases & heat is released 
b)
kinetic energy increases & heat is absorbed
15.
Water vapor (a gas) forming frost (a solid) on the windshield of a car is an example of what phase change?
a)
melting
b)
sublimation
c)
condensation
d)
deposition
16.

What criteria must be met for reactant collisions to result in a successful product?

a)

The reactants must collide with each other

b)

The reactants must collide with enough energy and be in the right positions

c)

The reactants must have enough energy to form the activated complex

17.

The energy needed by reactants for an effective collision is called the

a)

activation energy

b)

change in entropy

c)

change in enthalpy

d)

free energy

18.
The rate of a reaction increases as temperature__________________.
a)
Decreases
b)
Increases
c)
Stays the Same
19.

Products will form faster if____________

a)

the surface area of the reactants are smaller.

b)

temperature is decreased.

c)

concentration of the reactants are increased.

d)

the reaction is not stirred.

20.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
21.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
22.
What letter represents the activation energy?
a)
A
b)
B
c)
C
d)
D
23.

Why does a higher temperature increase the rate of a reaction?

a)

because it increases both the frequency and energy of particle collisions

b)

because it only increases the frequency of particle collisions

c)

because it only increases the energy of particle collisions

d)

because it reduces the activation energy of the reaction

24.

Adding a catalyst ___________ the activation energy.

a)

Raises

b)

Lowers

c)

Doesn't affect

d)

Inreases

25.

As the frequency of ______________ increases, the rate of reaction increases.

a)

Time

b)

Reactions

c)

Collisions

d)

Reactants

26.

What makes the explosion occur in a coal mine?

a)

Due to the certain concentration of fllammable small particles contact with air

b)

Due to the pressure of air

c)

Due to the certain temperature of flammable gas

d)

Due to the density of gas and air

27.

Why don't all collisions between particles cause a reaction?

a)

The particles also need to collide with a catalyst.

b)

Not all colliding with enough energy and correct orientation

c)

Not all particles collide at a high enough temperature.

d)

The particles need to collide with each other twice.

28.

According to the graph, it can be concluded that

a)

As reaction progresses, the concentration of product will reduce and the reactant will increase

b)

As reaction progresses, the concentration of product and reactant will reduce

c)

As reaction progresses, the concentration of product and reactant will increase

d)

As reaction progresses, the concentration of product will increase, the reactant will reduce

29.

All chemical reactions happen at the same speed.

a)

true

b)

false

30.
a)

K=[CO] [H2] 3 / [CH4] [H2O]

b)

K=[H2]3 [CO] /[CH4] [H2O]

c)

K=[CO] [H2] 3 /[H2O] [CH4]

d)

K=[H2]3[CH4] /[CO] H2O]

31.

The factors that effect a system at equilibrium except:

a)

Caltalyst

b)

Temperature

c)

Pressure and volume

d)

Mass

32.

What is the Keq expression for the following reaction:

PCl5(g) --> PCl3(g) + Cl2(g)

a)

Keq= [PCl3] [Cl2] / [PCl5]

b)

Keq=[PCl5] / [PCl3] [Cl2]

c)

Keq= [PCl3] + [Cl2] / [PCl5]

d)

Keq=[PCl5] / [PCl3] + [Cl2]

33.

Which of these conditions prevails (exists) at equilibrium?

a)

the forward reaction happens faster than the reverse reaction

b)

the forward reaction happens slower than the reverse reaction

c)

the forward reaction and reverse reaction happen at the same rate

d)

the forward reaction has stopped

34.

If Keq is greater than 1, the at equilibrium:

a)

the amount of product is greater than the amount of reactant (products favored)

b)

the amount of reactant is greater than the amount of product (reactants favored)

c)

the amount of reactant and product is equal

d)

the amount of product is zero

35.

What is the Keq expression for the following reaction:

2Na2O2(s) + 2CO2(g) --> 2Na2CO3(s) + O2(g)

a)

Keq= [O2] / [CO2]2

b)

Keq=[CO2]2/ [O2]

c)

Keq= [Na2CO3]2 [O2] / [Na2O2]2 [CO2]2

d)

Keq= [Na2CO3] [O2] / [Na2O2] [CO2]

36.

For the reaction 2SO2(g) + O2(g) --> 2SO3(g) at equilibrium, the removal of O2 would cause:

a)

the concentration of SO2 to increase and the concentration of SO3 to increase

b)

the concentration of SO2 to increase and the concentration of SO3 to decrease

c)

the concentration of SO2 to decrease and the concentration of SO3 to increase

d)

the concentration fo SO2 to decrease and the concentration of SO3 to decrease.

37.

A substance is found to have the following characteristics:


Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water


In what category would the substance be classified?

a)

acid

b)

base

c)

enzyme

d)

fatty acid

38.

KOH is ...

a)

an acid

b)

a base

c)

a salt

d)

an ionic compound

39.

What is the pH of a solution where the [H+] is 1.0 x 10-11?

a)

11

b)

13

c)

14

d)

1

40.

What is the [H+] if the pH is 4.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-4 M

c)

1.0 x 10-14 M

d)

1.0 x 10-7 M

41.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
42.

an acid is a substance that contains hydrogen and a base is a substance that contains a hydroxide group

a)

Arrhenius Model

b)

Bronsted-Lowery Model

c)

Lewis Model

d)

Neutralization

43.

an acid that ionizes completely in aqueous solution

a)

strong acid

b)

weak acid

c)

strong base

d)

weak base

44.

a reaction in which an acid and a base react to produce a salt and water

a)

Arrhenius model

b)

neutralization

c)

single replacement reaction

d)

Bronsted-Lowery model

45.

What is the proper chemical formula for phosphoric acid?

a)

H3PO

b)

H3PO4

c)

HPO4

d)

HPO2

46.

The pH of a solution prepared by mixing equal amounts of 0.125M KOH and 0.125M HCl is

a)

6.29

b)

0.00

c)

7.00

d)

5.78

47.

The correct name for H2SO4 is _____________ acid

a)

hydrosulfuric

b)

hydrosulfurous

c)

sulfurous

d)

sulfuric

48.

What is the concentration of hydronium ions in a solution with a pH of 4.282

a)

0.5224M

b)

5.224 x 10-5M

c)

0.05224M

d)

5.224M

49.

What is the pH of a solution with a concentration of 0.050M HNO3?

a)

0.00

b)

1.30

c)

5.24

d)

7.00

50.

Which type of reaction is:

3 Pb + 2 H3PO4 → 3 H2 + Pb3(PO4)2

a)
Synthesis
b)
Single Displacement
c)
Double Displacement
d)
Combustion
51.

Balance the following:

____ H2SO4 + ____ NaNO2 → ____ HNO2 + ____ Na2SO4

a)
1,1,2,1
b)
1,2,2,1
c)
2,3,3,2
d)
4,3,2,1
52.

Which type of reaction is:

2 NH3 + H2SO4 → (NH4)2SO4

a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
53.

Which type of reaction is:

3 Pb + 2 H3PO4 → 3 H2 + Pb3(PO4)2

a)
Synthesis
b)
Single Displacement
c)
Double Displacement
d)
Combustion
54.

N4O9

a)

Tetranitride nonoxide

b)

Tetranitrogen nonaoxide

c)

Tetranitrogen nonoxide

55.

Which type of reaction is:

3 Pb + 2 H3PO4 → 3 H2 + Pb3(PO4)2

a)
Synthesis
b)
Single Displacement
c)
Double Displacement
d)
Combustion
56.

How many moles of CO2CO_2 are produced when 5.0 moles of C8H18C_8H_{18} are completely combusted in excess oxygen? (Balanced equation: 2C8H18+25O2→16CO2+18H2O2C_8H_{18} + 25O_2 \rightarrow 16CO_2 + 18H_2O )

a)

20 moles

b)

40 moles

c)

80 moles

d)

160 moles

57.

In the reaction 2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O , if 4 moles of H2H_2 are reacted with 2 moles of O2O_2 , which is the limiting reactant?

a)

H2H_2

b)

O2O_2

c)

Both react in exact stoichiometric proportions.

d)

Neither, as there is an excess of both reactants.

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