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Chemistry Second Semester Final

Total questions: 70

Worksheet time: 3hrs 33mins

Name
Class
Date
1.

What is the molar mass (NH4)2CO3?

a)

43.03 g/mol

b)

78.06 g/mol

c)

94.09 g/mol

d)

96.11 g/mol

2.

Find the percentage composition of Ni2(SO4)3.

a)

54.97%N 30.04%S 14.99%O

b)

50.00%Ni 33.33%S 8.33%O

c)

14.01%Ni 32.07%S 16%O

d)

28.94%Ni 23.72%S 47.34%O

3.
What is the molecular formula if the empirical formula is C2H5 and the molecular molar mass is 58.14 g/mol?
a)
C2H5
b)
C4H10
c)
C1H2.5
d)
C4H8
4.
2 CO (g) + O2(g) → 2 CO2 (g)
In the formation of CO2 from CO and oxygen, how many Liters of CO2 are produced by the reaction of 8 mols of O2 with an excess of carbon monoxide?
a)
0.178 L
b)
358.4 Liters
c)
704 grams
d)
0.36 grams
5.
What is Avogadro's Number? 
a)
6.02 x 1023
b)
- 6.02 1023
c)
6.02 x 1022
d)
6,020,000,000,000
6.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
7.
How do we get mass from moles?
a)
multiply by avogadro's number
b)
multiply by molar mass
c)
divide by avogadro's number
d)
divide by molar mass
8.
Which of the following is an empirical formula?
a)
C3H3
b)
Li2CO3
c)
Na2O2
d)
C6H12O6
9.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
10.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
11.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
12.

2 CO (g) + O2(g) → 2 CO2 (g)

In the formation of CO2 from CO and oxygen, how many Liters of CO2 are produced by the reaction of 8 mols of O2 with an excess of carbon monoxide?

a)

0.178 L

b)

358.4 L

c)

704 L

d)

0.36 L

13.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
14.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
15.

Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.

Mg + 2HCl --> MgCl2 + H2

a)

Mg

b)

H2

c)

MgCl2

d)

HCl

16.
A reaction was predicted to produce 32.4 grams of a compound. When the product was measured, there were only 26.1 grams made. What is the percent yield?
a)
80.6%
b)
6.3%
c)
24.1%
d)
58.5%
17.
Silver nitrate and sodium phosphate are reacted in equal amounts of 200 g each. How many grams of silver phosphate are produced? 
3AgNO3  + Na3(PO4)  --->  Ag3(PO4)  + 3NaNO3
a)
164 g
b)
64 g
c)
146 g
d)
164 moles
18.
Your percent yield is 80%. The actual amount of product produced was 29.1 grams. What is the theoretical yield?
a)
25.2 grams
b)
37.3 grams
c)
37.1 grams
d)
36.3 grams
19.

The limiting reactant is the reactant that __________ .

a)

slows down the reaction

b)

used up first

c)

left over at the end of reaction

d)

controls the speed of the reaction

20.
How many water molecules are in 5.2 moles of water?
a)
6.02 x 1023
b)
5.2
c)
3.1304 x 1024
d)
8.638 x 10-24
21.

Which of the following is not a physical property of gases?

a)

absence of definite volume

b)

large density

c)

high compressibility

d)

fluidity

22.

Which one of these is NOT an Ideal Gas Assumption?

a)

Gas particles are hard, round spheres.

b)

Gas particles are strongly attracted to one another.

c)

Gas particles do not take up space.

d)

Gas particles collide perfectly elastically.

23.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

24.
What about gases can be measured?
a)
Pressure and Volume
b)
Temperature, Volume, and Pressure
c)
Volume and Temperature
d)
Pressure, Temperature, Volume, and Moles
25.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
26.

Pressure is

a)

defined as the mass that an object exerts when at rest.

b)

not a measurable in gases.

c)

defined as the number of moles of substance divided by the mass of the substance.

d)

created by the force of the gas particles impacting the walls of the container.

27.

What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?

a)

3670 atm

b)

0.245 atm

c)

4.08 atm

d)

605 atm

28.

If 3.0 L of helium at 293 K with a pressure of 200 kPa is allowed to expand to 4.4 L with the pressure staying constant. What is the new temperature?

a)

702 K

b)

430 K

c)

157 K

d)

0 K

29.

Use Graham’s Law to calculate fast O2 gas will effuse compared to Cl2.

a)

O2 effuses 1.5 times faster than Cl2

b)

O2 effuses 0.67 times as fast as Cl2

c)

O2 effuses 2.2 times faster than Cl2

d)

O2 effuses 0.45 times as fast as Cl2

30.

A sample of carbon dioxide experiences a change in volume from 54.16 L to 22.323 L. If its new pressure is 554.05 kPa, what was its original pressure in kilopascals?

(a)  

31.

While making homemade ice cream, you add rock salt to the ice. Which choice below provides the best explanation for why this is done?

a)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is lower than just the ice.

b)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is higher than just the ice.

c)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is lower than just the ice.

d)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is higher than just the ice.

32.
What is the freezing point of an antifreeze solution created by adding 651 g of ethylene glycol (CH2(OH)CH2(OH)) to 2505 g of water? Kf = 1.86 oC/m
a)
-4.19 oC
b)
2.2 oC
c)
0 oC
d)
-7.79 oC
33.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
34.

What is the percent concentration of sugar in pink lemonade if 28 g of sugar is added to 209 g of water?

a)

14.7 %

b)

5.14 %

c)

13.4 %

d)

11.8 %

35.

What is the boiling point of a 1.50 m NaCl solution? (Kb=0.512 degrees C/m)

a)

100 degrees Celsius

b)

105.2 degrees Celsius

c)

101.5 degrees Celsius

d)

102.8 degrees Celsius

36.

What is the molality of a solution made by dissolving 2 moles of NaOH in 400 grams of water?

a)

5 mol/kg. solvent

b)

4 mol/kg solvent

c)

3 mol/kg. solvent

d)

2.5 moles /kg solvent

37.

As per Henry law, Solubility of a gas in a liquid is directly proportional to __________ of the gas.

a)

temperature

b)

pressure

c)

volume

d)

pressure x volume

38.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

39.

The process of dissolving a substance in solution

a)

solvotion

b)

salvation

c)

solvation

d)

salvution

40.

What does "like dissolves like" mean?

a)

polar solvents dissolve in polar solutes

b)

polar solutes dissolve in polar solvents

c)

non-polar solvents dissolve in polar solutes

d)

non-polar solutes dissolve in polar solvents

41.

If the Keq = 0.65

a)

the forward reaction is favored

b)

the reverse reaction is favored

c)

the reaction will simultaneously favor the forward and reverse

d)

not enough information is given

42.

2 H2S <------> 2 H2 + S2

When the contents were analyzed they were 0.6 mole of H₂S and 0.80 mole S₂ in a 1L container and Keq = 0.016. What is the concentration of H2?

a)

0.007

b)

0.08

c)

0.04

d)

0.2

43.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
44.
For the reaction...
N2 (g) +  3 H2 (g) <=> 2 NH3 (g)

If the pressure in the system is increased,  which substance(s) will increase in concentration?
a)
N2  (as 2 mol gas  → 4 mol gas)
b)
H2 (as 2 mol gas  → 4 mol gas)
c)
N2 and H2 (as 2 mol gas  → 4 mol gas)
d)
NH3 (as 4 mol gas  → 2 mol gas)
45.
Consider the following reaction:
2SO2(g) + O2(g) <=> 2SO3(g):  ΔΗ = - 197 kJ mol -1
Which of the following will NOT shift the equilibrium position to the right?
a)
Adding more O2
b)
Adding a catalyst
c)
increasing the pressure
d)
Lowering the temperature
46.
The following reaction :    
SO2 (g) +  NO2 (g) <=> SO3 (g) + NO (g)  
had reached a state of equilibrium, was found to contain  
0.40 mol L-1 SO3 , and 0.30 mol L-1 NO,
0.15 mol L-1NO2 , and 0.20 mol L-1 SO2.
Calculate the equilibrium constant  for this reaction. 
a)
4
b)
.42
c)
.25
d)
1
47.

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]

48.

A possible mechanism for reaction :


A + 2B → C + D


is shown below :


2B → E (slow)

A + E → C + D (fast)


which of the following diagram represents reaction pathway diagram for this reaction mechanism?

a)
b)
c)
d)
49.
Find the order for F2 and CIO2 using data shown below.
a)
(F2 - 2nd order) (CIO2 - 1st order)
b)
(F2 - 1st order) (CIO2 - 1st order)
c)
(F2 - 1st order) (CIO2 - 2nd order)
d)
(F2 - 2nd order) (CIO2 - 2nd order)
50.
What is the rate exponent for A?
a)
0
b)
1
c)
2
51.

What is the formula for the following acid: Chloric Acid

a)

HCl

b)

HClO2

c)

HClO3

d)

HC

52.

If a solution has a [H+] of 1.0 x 10 -5, what is the [OH-]?

a)

1.0 x 10 -9

b)

1.0 x 10 -5

c)

1.0 x 10 -14

d)

1.0 x 10 -7

53.

What does a color change to faint pink signal in a titration?

a)

End point has been reached and solution is neutralized.

b)

Solution is more acidic

c)

You need to add more base.

d)

The pH of the solution is 14

54.

During a titration, 20. mL of 0.50 M HF is used to neutralize 10. mL of NaOH. What is the concentration of the base?

a)

1.0 M NaOH

b)

0.25 M NaOH

c)

400 M NaOH

d)

10 M NaOH

55.

Human blood has a pH between 7.35 and 7.45. Which of the following is a solution in which the pH remains relatively constant when small amounts of acid or base are added.?

a)

catalyst

b)

salt solution

c)

buffer

d)

inhibitor

56.

What type of salt produces an acidic solution?

a)

strong acid + weak base

b)

strong acid + strong base

c)

weak acid + weak base

d)

weak acid + strong base

57.

What is the color of litmus paper in an acid?

a)

Pink

b)

Blue

c)

Red

d)

Colorless

58.
What is the [OH-] if the pH is 4.9?
a)
7.94 x 10-10 M
b)
1.0 x 10-4  M
c)
7.94 x 10-14 M
d)
4.9 x 10-10 M
59.

If we dissolve 20.0 grams of HCl in 1.2 L of water, what is the pH of that solution?

a)

0.34

b)

4.21

c)

7.20

d)

10.34

60.
The following statement is true for arrhenius acid and base EXCEPT
a)
Arrhenius acid produces H+ ions
b)
Arrhenius base produces OH- ions
c)
H2O need to be present for arrhenius acid base to dissociate
d)
Hydrogen atoms that make the solution acidic
61.

What is the oxidation number assigned to manganese in KMnO4?

a)

+7

b)

+2

c)

+4

d)

+3

62.

In which substance does sulfur have a negative oxidation number?

a)

S

b)

CaSO4

c)

Na2S

d)

SO2

63.

In a redox reaction, the species reduced

a)

gains electrons and is the oxidizing agent

b)

loses electrons and is the oxidizing agent

c)

loses electrons and is the reducing agent

d)

gains electrons and is the reducing agent

64.

- What is the oxidation number of chromium in K2Cr2O7

a)

+6

b)

+3

c)

+5

d)

+2

65.
Which statement is true:
Mg → Mg2+ + 2e–
a)
Mg gains 2 electrons
b)
Mg2+ loses 2 electrons
c)
Mg loses 1 electron
d)
Mg loses 2 electrons
66.
What substance is oxidized in the following reaction?
4Fe + 3O2 --> 2Fe2O3
a)
Iron
b)
Fluorine
c)
Oxygen
67.

In which substance does hydrogen have an oxidation number of zero?

a)

LiH

b)

H2O

c)

H2S

d)

H2

68.

Given the reaction:


F2(g) + 2 Br–(aq) → Br2() + 2 F–(aq)


Which species is reduced?

a)

F2(g)

b)

Br–(aq)

c)

Br2 (l)

d)

F–(aq)

69.

Identify the substance that is reduced in the reaction between copper(II) ion and magnesium.

Cu2+ + Mg → Cu + Mg2+

a)

Cu2+

b)

Mg

c)

Cu

d)

Mg2+

70.

Cl2 + 2e- --> 2Cl - is an example of:

a)

a chemical reaction

b)

redox

c)

oxidation

d)

reduction

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