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ACP Chemistry Final Review

Total questions: 60

Worksheet time: 1hrs 7mins

Name
Class
Date
1.

How many valence electrons does a neutral atom of oxygen have?

a)

4

b)

6

c)

2

d)

8

2.

Which of the following correctly represents a magnesium ion?

a)

Mg+2

b)

Mg+1

c)

Mg-1

d)

Mg-2

3.

What is the chemical formula for beryllium phosphate?

a)

Be2(PO4)3

b)

Be3(PO4)2

c)

BeP

d)

BePO4

4.

What is the molar mass of ammonium sulfate, (NH4)2SO4?

a)

114.11 g/mol

b)

63.08 g/mol

c)

132.16 g/mol

d)

528.64 g/mol

5.

Which set of coefficients would balance the following chemical reaction?


_AlCl3 + _NaOH --> _NaCl + _Al(OH)3

a)

3,1,1,3

b)

1,3,3,1

c)

1,1,1,1

d)

1,3,1,1

6.

What is the mass of a 4.3 mol sample of Ca(NO3)2?

a)

164.09 g

b)

705.6 g

c)

70 g

d)

710 g

7.

Consider the reaction

2H2O2(aq) --> 2H2O(l) + O2(g)


What happens to the mass of the system as the reactants are converted to products?

a)

It stays the same

b)

It decreases

c)

It increases

d)

Not enough info given

8.

Consider the reaction

CaCl2 + 2AgNO3 --> 2AgCl + Ca(NO3)2


If 2.0 mol of CaCl2 is mixed with 5.0 mol of AgNO3, what will be the limiting reagent/reactant?

a)

AgCl

b)

CaCl2

c)

AgNO3

d)

Ca(NO3)2

9.

Consider the reaction

CaCl2 + 2AgNO3 --> 2AgCl + Ca(NO3)2


If 4 mol of AgNO3 react completely according to the equation, how many moles of Ca(NO3)2 will be produced?

a)

2

b)

4

c)

1

d)

8

10.

At constant temperature and volume, decreasing the number of moles of gas decreases the pressure of the sample because

a)

The number of collisions decreases

b)

The mass of the sample decreases

c)

The kinetic energy of the gas molecules decreases

d)

The kinetic energy of the gas molecules increases

11.

A 3.00 L sample of gas is at a temperature of 250. K and a pressure of 3.00 atm. If the temperature is doubled to 500. K at a constant volume, what will be the final pressure of the gas?

a)

6.00 atm

b)

4.50 atm

c)

1.50 atm

d)

3.00 atm

12.

What is the volume of a 1.24 mol sample of nitrogen gas held at a temperature of 82°C and a pressure of 2.50 atm?

a)

14.4 L

b)

58.7 L

c)

3.34 L

d)

13.6 L

13.

What is the volume occupied by 2.3 moles of argon gas at STP?

a)

2.3 L

b)

9.7 L

c)

52 L

d)

0.10 L

14.

Which of the following is NOT an example of a phase change?

a)

Combustion

b)

Evaporation

c)

Freezing

d)

Melting

15.

What is the melting point of this substance?

a)

90°C

b)

35°C

c)

120°C

d)

55°C

16.

At which of the following temperatures is this material present only in the solid state?

a)

100°C

b)

70°C

c)

40°C

d)

60°C

17.

During an endothermic process

a)

No heat transfer occurs

b)

Heat is gained by the system

c)

Heat is lost by the system

d)

∆H is a negative number

18.

The heat of fusion of iron is 247 J/g. How many grams of Fe can be melted by 6175 J of heat?

a)

1.53x106 g

b)

25.0 g

c)

50.0 g

d)

0.0400 g

19.

What is the oxidation state of the phosphorous atom in the phosphate ion, PO4-3

a)

-5

b)

-3

c)

+8

d)

+5

20.

In the chemical reaction


NH3 + O2 --> NO + H2O


Which element is reduced?

a)

Hydrogen, H

b)

Nitrogen, N

c)

Oxygen, O

d)

None of the above

21.

How many valence electrons are there in a neutral atom of aluminum?

a)

13

b)

2

c)

3

d)

8

22.

What is the electron configuration of scandium, Sc?

a)

1s22s22p63s23p64s24d1

b)

1s22s22p63s23p64s23d1

c)

1s22s22p63s23p64s3

d)

1s22s22p63s23p4

23.

Which element is an exception to the octet rule?

a)

O

b)

B

c)

C

d)

N

24.

Which of the following elements is the most electronegative?

a)

B

b)

Rb

c)

F

d)

C

25.

Which pair or elements represents a polar covalent bond?

a)

Na-F

b)

F-F

c)

C-F

d)

Al-F

26.

Which of the following is the weakest of the intermolecular forces?

a)

London Dispersion

b)

Dipole-dipole

c)

Ionic Bonding

d)

Hydrogen Bonding

27.

A sample of CuSO4 is being dissolved in water. Which of the following actions would NOT speed up the dilution process?

a)

Stir the solution

b)

Put the solution on ice

c)

Grind up the solute before adding it to the solvent

28.

How many grams of NH4Cl will dissolve in 100 g of water at 40°C?

a)

75 g

b)

35 g

c)

30 g

d)

45 g

29.

A chemist dissolves 70 g of NaNO3 in 100 g of water at 30°C. This solution is:

a)

Supersaturated

b)

Unsaturated

c)

Saturated

d)

None of the options

30.

A 6.75 mol sample of NaCl is dissolved in 850. mL of water. What is the molarity of the resulting solution?

a)

6.75 M

b)

0.00794 M

c)

7.94 M

d)

5.74 M

31.

If 2.0 L of a 4.30 M Mg(OH)2 solution are diluted to a volume of 6.25 L, what would be the final concentration?

a)

13 M

b)

2.9 M

c)

1.4 M

d)

1.3 M

32.

When running a chemical reaction, increasing the concentrations of the reactants will

a)

Have no effect on the rate of reaction

b)

Increase the rate of reaction

c)

Decrease the rate of reaction

d)

Increase the temperature of the reaction

33.

How does a catalyst speed up a reaction?

a)

Lowering the activation energy (Ea)

b)

Raising the activation energy (Ea)

c)

Lowering the enthalpy of reaction (∆H)

d)

Lowering the energy of the reactants

34.

What is the activation energy for the reaction?

a)

40 kJ

b)

20 kJ

c)

70 kJ

d)

-70 kJ

35.

What is the enthalpy of reaction (∆H) of this reaction?

a)

40 kJ

b)

-40 kJ

c)

-30 kJ

d)

30 kJ

36.

This reaction is...

a)

Endothermic

b)

Exothermic

c)

Isothermic

d)

Not enough information given

37.

Consider the reaction


3Cl2(g) + CS2(g) ⇌ CCl4(g) + S2Cl2(g)


If this system is at equilibrium, adding CCl4 will

a)

Shift the equilibrium to the left

b)

Change the Keq of this system

c)

Have no effect on the equilibrium

d)

Shift the equilibrium to the right

38.

What is the equilibrium constant expression for the reaction?


3Cl2(g) + CS2(g) ⇌ CCl4(g) + S2Cl2(g)

a)
b)
c)
d)
39.

Which of the following is an acid?

a)

NaOH

b)

H3PO4

c)

C2H6

d)

Na3PO4

40.

What is the pH of a 2.1x10-2 M NaOH solution?

a)

2

b)

12.3

c)

4.76

d)

1.7

41.

Which of the following represents a basic solution?

a)

pH = 1

b)

pH = 5

c)

pH = 7

d)

pH = 9

42.

What is the hydrogen ion concentration, [H+], of a solution with a pH of 6.3?

a)

2.0x10-8 M

b)

5.01x10-7 M

c)

6.3x100 M

d)

2.0x106 M

43.

What volume of a 1.50 M HCl solution would be needed to neutralize 0.45 L of 0.80 M KOH?

a)

0.24 L

b)

0.54 L

c)

0.84 L

d)

0.38 L

44.

What nuclear reaction is represented by the following equation?

a)

Fission

b)

Fusion

c)

Beta Decay

d)

Alpha Decay

45.

Determine the identity of the missing isotope in the following nuclear reaction.

a)
b)
c)
d)
46.

How much energy is released when 50.5 g of trichloromethane cools from 37.9°C to 30.0°C? The specific heat of trichloromethane is 0.971 J/g°C.

a)

-1858 J

b)

-1471 J

c)

-387J

d)

.0024 J

47.

Given the following equation:


_C3H8 + _O2 --> _CO2 + _H2O


What coefficients would balance the equation?

a)

1,1,1,1

b)

1,2,2,1

c)

2,3,5,2

d)

1,5,3,4

48.

Using the balanced equation from the previous question, if 30.0 g of C3H8 are allowed to react with 89.6 g of O2, what will be the limiting reagent?

a)

C3H8

b)

O2

c)

CO2

d)

H2O

49.

Using the limiting reagent from the previous question, what mass of water can theoretically be produced?

a)

40.3 g

b)

49.0 g

c)

2.24 g

d)

2.72 g

50.

Using the mass of water produced from the previous question and assuming that 36.7 g of water are actually collected after the reaction, what is the percent yield for this experiment?

a)

40.3%

b)

74.9%

c)

36.7%

d)

91.1%

51.

What is the correct Lewis dot structure for PF3?

a)

a

b)

b

c)

c

d)

d

52.

What is the correct dot diagram for CH2Cl2?

a)

a

b)

b

c)

c

d)

d

53.

What is the correct dot diagram for CS2?

a)

a

b)

b

c)

c

d)

d

54.

Given the following equation, what is the correct Keq?


4H2 (g) + O2 (g) <--> 2H2O + 780 kJ

a)

Keq = [H2O]2 / [H2]4 + [O2]

b)

Keq = [H2O]2 / [H2]4 x [O2]

c)

Keq = [H2]4 x [O2] / [H2O]2

d)

Keq = [H2]4 + [O2] / [H2O]2

55.

Given the following reaction:

4H2 (g) + O2 (g) <--> 2H2O + 780 kJ

Removing one of the reactants would cause the equilibrium to shift in which direction?

a)

Left

b)

Right

c)

No Shift

d)

Not enough information given

56.

Given the following reaction:


4H2 (g) + O2 (g) <--> 2H2O + 780 kJ


If the system shifts towards the right, what would happen to the temperature of the system?

a)

Increase

b)

Decrease

c)

Stays the same

d)

Not enough information given

57.

Given the following reaction:


4H2 (g) + O2 (g) <--> 2H2O + 780 kJ


What happens to the Keq of this system when the [H2O] decreases?

a)

Increases

b)

Decreases

c)

Stays the same

d)

Not enough information provided

58.

Given the following information, calculate the molarity of the unknown acid:

a)

1.0 M

b)

0.25 M

c)

2.0 M

d)

0.51 M

59.

The reaction between an acid and a base,


HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq)


is called a(n)

a)

Composition reaction

b)

Neutralization reaction

c)

Redox reaction

d)

Single ionic replacement reaction

60.

What type of reaction is represented by the following equation?


Mg + 2HCl --> H2 + MgCl2

a)

Composition/Synthesis/Combination

b)

Decomposition

c)

Single Ionic Replacement (SIR)

d)

Double Ionic Replacement (DIR)

e)

Combustion

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