Free Printable Chemistry Second Semester Review: Units 4-9

1.

In the equation $2\ Al_2O_{3\ }\rightarrow\ 4\ Al\ \ +\ \ 3\ O_2$ , what is the mole ratio of aluminum to oxygen?

a)

10:6

b)

3:4

c)

2:3

d)

4:3

2.

The limiting reactant of a reaction can be used to calculate the

a)

actual yeild.

b)

theoretical yield.

c)

experimental yield.

d)

Both (a) and (c).

3.

The coefficients in a chemical equation represent the

a)

masses, in grams, of all reactants and products.

b)

numbers of moles of reactants and products.

c)

number of atoms in each compound in a reaction.

d)

number of valence electrons involved in the reaction.

4.

The units of molar mass are

a)

g/mol.

b)

mol/g.

c)

amu/mol.

d)

amu/g.

5.

For the reaction represented by the equation

$2\ H_2\ \ +\ \ O_2\ \rightarrow\ 2\ H_2O$ , how many moles of water

can be produced from

6.0 mol of oxygen?

a)

2.0 ml

b)

6.0 mol

c)

12 mol

d)

18 mol

6.

Which observation DOES NOT indicate that a chemical reaction has occurred?

a)

formation of a precipitate

b)

production of a gas

c)

evolution of heat and light

d)

change in total mass of substances

7.

When a solid produced by a chemical reaction separates from the solution it is called

a)

a precipitate.

b)

a reactatnt.

c)

a molecule.

d)

the mass of the product.

8.

According to the law of conservation of mass, the total mass of the reacting substances is

a)

always more than the total mass of the products.

b)

always less than the total mass of the products.

c)

sometimes more and sometimes less than the total mass of the products.

d)

always equal to the total mass of the products.

9.

Which coefficients correctly balance the formula equation?

$NH_4NO_3\ \left(s\right)\ \ \rightarrow\ \ N_{2_{ }}\left(g\right)\ \ +\ \ H_2O\ \left(l\right)$

a)

1, 2, 2

b)

1, 1, 2

c)

2, 1, 1

d)

2, 2, 2

10.

What is the balanced equation for the combustion of sulfur?

a)

$S\left(s\right)\ \ +\ \ O_2\left(g\right)\ \ \rightarrow\ SO\left(g\right)$

b)

$S\left(s\right)\ +\ O_2\left(g\right)\ \ \rightarrow\ SO_2\left(g\right)$

c)

$2\ S\left(s\right)\ +\ 3\ O_2\left(g\right)\rightarrow\ SO_3\left(s\right)$

d)

$S\left(s\right)+2\ O_2\ \left(g\right)\rightarrow SO_4^{-2}\left(aq\right)$

11.

The reaction represented by the equation

$2\ Mg\left(s\right)\ +\ O_2\left(g\right)\rightarrow2\ MgO\left(s\right)$

is a

a)

synthesis reaction.

b)

decomposition reaction.

c)

single-displacement reaction.

d)

double-displacement reaction.

12.

The reaction represented by the equation

$Mg\ +\ 2\ HCl\ \rightarrow\ H_2\ +\ MgCl_2$

is a

a)

composition reaction.

b)

decomposition reaction.

c)

single-displacement reaction.

d)

double-displacement reaction.

13.

The reaction represented by the equation $Pb\left(NO_3\right)_2\ +\ 2KI\ \rightarrow\ PbI_2\ +\ 2KNO_3$

a)

double-displacement reaction.

b)

synthesis reaction.

c)

decomposition reaction.

d)

combustion reaction.

14.

What can be predicted by using an activity series?

a)

whether a certain chemical reaction will occur

b)

the amount of energy released by a chemical reaction

c)

the electronegativity values of elements

d)

the melting points of elements

15.

According to the kinetic-molecular theory, particles of matter

a)

are in constant motion.

b)

have different shapes.

c)

have different colors.

d)

are always fluid.

16.

What determines the average kinetic energy of the molecules of any gas?

a)

temperature

b)

pressure

c)

container volume

d)

molar mass

17.

What happens to the volume of a gas during compression?

a)

The volume increases.

b)

The volume decreases.

c)

The volume remains constant.

d)

It is impossible to tell because all gases are different.

18.

The particles in a liquid are usually

a)

closer together and lower in energy than those in a solid.

b)

farther apart and higher in energy than those in a gas.

c)

closer together and lower in energy than those in a gas.

d)

farther apart and lower in energy than those in a solid.

19.

The energy of the particles in a solid is

a)

higher than the energy of the particles in a gas.

b)

high enough to allow the particles to interchange with other particles.

c)

higher than the energy of the particles in a liquid.

d)

lower than the energy of the particles in liquids and gases.

20.

Solids have a definite volume because

a)

the particles do not have a tendency to change positions.

b)

the particles are far apat.

c)

they can be easily compressed.

d)

the energy of the particles is high.

21.

A heterogeneous mixture always contains

a)

only one substance.

b)

more than two substances.

c)

two or more substances that are visibly distinguishable.

d)

two or more substances that are not visibly distinguishable.

22.

Carbon dioxide dissolved in water is an example of which solute-solvent combination?

a)

gas-liquid

b)

liquid-gas

c)

liquid-liquid

d)

cannot be determined

23.

Sugar dissolved in water is an example of which solute-solvent combination?

a)

gas-liquid

b)

liquid-liquid

c)

solid-liquid

d)

liquid-solid

24.

Oxygen in nitrogen is an example of which solute-solvent combination?

a)

gas-liquid

b)

liquid-gas

c)

gas-solid

d)

gas-gas

25.

A metal solution is a(n)

a)

colloid.

b)

alloy.

c)

suspension.

d)

emulsion.

26.

Which of the following is an electrolyte?

a)

sodium chloride

b)

sugar

c)

pure water

d)

glass

27.

Which of the following will dissolve most rapidly?

a)

sugar cubes in cold water

b)

sugar cubes in hot water

c)

powdered sugar in cold water

d)

powdered sugar in hot water

28.

In the expression "like dissolves like," the word like refers to similarity in molecular

a)

mass.

b)

size.

c)

energy.

d)

polarity.

29.

Which of the following is an example of a polar solvent?

a)

carbon tetrachloride

b)

benzene

c)

water

d)

gasoline

30.

Two immiscible substances

a)

exist together in one phase.

b)

will not separate on standing.

c)

dissolve freely in one another in any proportion.

d)

will not form a solution.

31.

What does the constant bombardment of gas molecules against the inside walls of a container produce?

a)

temperature

b)

density

c)

pressure

d)

diffusion

32.

The reaction represented by the equation 2 HgO (s) → 2 Hg (l) + O₂ (g) is a(n)

a)

single-displacement reaction.

b)

synthesis reaction.

c)

combustion reaction.

d)

decomposition reaction.

33.

Acids taste

a)

sweet.

b)

sour.

c)

bitter.

d)

salty.

34.

Acids generally release H₂ gas when they react with

a)

nonmetals.

b)

semimetals.

c)

active metals.

d)

inactive metals.

35.

Acids react with

a)

bases to produce salts and water.

b)

salts to produce bases and water.

c)

water to produce bases and salts.

d)

neither bases, salts, nor water.

36.

Bases taste

a)

soapy.

b)

sour.

c)

sweet.

d)

bitter.

37.

Which acid is produce in the stomach?

a)

Hydrochloric

b)

Phosphoric

c)

Nitric

d)

Sulfuric

38.

What is the pH of a neutral solution at 25 degrees Celsius?

a)

0

b)

1

c)

7

d)

14

39.

The pH scale in general ranges from

a)

0 to 1.

b)

-1 to 1.

c)

0 to 7.

d)

0 to 14.

40.

The pH of an acidic solution is

a)

less than 0.

b)

less than 7.

c)

greater than 7.

d)

greater than 14.

41.

The pH of a basic solution is

a)

less than 0.

b)

less than 7.

c)

greater than 7.

d)

greater than 14.

42.

What is the pH of a 10^-4 M HCl solution?

a)

4

b)

6

c)

8

d)

10

43.

How would you classify HCl, in the equation below?

HCl (aq) x H₂O (l) → H₃O⁺ (aq) + Cl^- (aq)

a)

a weak acid

b)

a strong acid

c)

a weak base

d)

a strong base

44.

How would you classify CH₃COOH in the equation below?

CH₃COOH (aq) + H₂O (l) ↔ H₃O⁺ (aq) + CH₃CO^-(aq)

a)

a weak acid.

b)

a strong acid.

c)

a weak base.

d)

a strong base.

45.

The pH of a solution is 9.0. What is its H⁺ concentration?

a)

1 x 10 ^-9 M

b)

1 x 10^-7 M

c)

1 x 10^-5 M

d)

9 M

46.

An acid-base titration involves a

a)

composition reaction.

b)

neutralization reaction.

c)

single-displacement reaction.

d)

decomposition reaction.

47.

During an acid-base titration, a very rapid change in pH

a)

occurs when the first addition of the known solution is made.

b)

occurs when the amounts of H⁺ ions and OH^- ions are nearly equivalent.

c)

occurs at several points during the titration.

d)

does not occur during titration.

48.

When titrating a strong acid with a strong base, the equivalence point

a)

will be below a pH of 7.0.

b)

will be above a pH of 7.0.

c)

will be at a pH of 7.0.

d)

will be either above or below a pH of 7.0.

49.

A reaction in which products can react to re-form reactants is

a)

reforming.

b)

reversible.

c)

buffered.

d)

impossible.

50.

At equilibrium,

a)

the forward reaction rate is lower than the reverse reaction rate.

b)

the forward reaction rate is higher than the reverse reaction rate.

c)

the forward reaction rate is equal to the reverse reaction rate.

d)

no reactions take place.

Chemistry Second Semester Review: Units 4-9

Total questions: 50

Worksheet time: 41mins

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