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Chemistry: Semester 2 Review

Total questions: 100

Worksheet time: 5hrs 30mins

Name
Class
Date
1.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

2.

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

3.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.1 atm

c)

1.6 atm

d)

3.4 atm

4.

Three gases are mixed together in a container with a total pressure of 4.8 atm. If two of the gases have pressures of 1.2 atm and 1.5 atm, what is the pressure of the third gas?

a)

2.5 atm

b)

1.8 atm

c)

2.1 atm

d)

1.3 atm

5.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
6.
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
7.
What is 50 °C in Kelvin?
a)
223
b)
323
c)
100
d)
50
8.
Charles' Law States...
a)
As Pressure goes up volume goes down
b)
As Pressure goes up temperature goes up
c)
As Volume goes up temperature goes up 
d)
As Pressure goes down volume goes down 
9.
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
10.

Determine the temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure.

a)

0 K

b)

107 K

c)

207 K

d)

307 K

11.

A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?

a)

60.0 mL

b)

15.0 mL

c)

27.5 mL

d)

32.5 mL

12.

When Volume of a gas increases, the Pressure will ______________

a)

Increase

b)

Decrease

c)

Stay the Same

13.

When Temperature of a gas increases, the Pressure will ____________________

a)

Increase

b)

Decrease

c)

Stay the Same

14.

What is the Standard for Temperature and Pressure?

a)

273 K and 1 atm

b)

273 C and 1 kPa

c)

273 F and 1 mmHg

d)

273 K and 1 Torr

15.

The pressure inside a tire is 225 kPa. Express this value in atm.

a)

22792.5 atm

b)

171000 atm

c)

2.22 atm

d)

0.296 atm

16.

The pressure inside a tire is 225 kPa. Express this value in mm Hg.

a)

22792.5 mm Hg

b)

171000 mm Hg

c)

2.22 mm Hg

d)

1688 mm Hg

17.

The pressure of a gas is 725 mm Hg. Convert this into units of atm.

a)

551000 atm

b)

0.9539 atm

c)

73442.5 atm

d)

7.157 atm

18.
How many Joules of energy are required to change 10 gram of ice at -2 C to water at 20 C?
a)
440 J
b)
880 J
c)
10,140 J
d)
66,000 J
19.
What is the change in temperature when 50,000 Joules of energy is added to 200 grams of water at 25 C?
a)
0.016 C
b)
1,500 C
c)
63 C
d)
0.4 C
20.
How many Joules of energy are required to change 10 gram of water from 20 C to 90 C?
a)
1400 J
b)
2800 J
c)
210,000 J
d)
1,400,000 J
21.

What is the equation for specific heat capacity?

a)

Q=mcΔTQ=mc\Delta T

b)

Q=mcΔTQ=\frac{mc}{\Delta T}

c)

Q=ΔTmcQ=\frac{\Delta T}{mc}

d)

Q=cΔTmQ=\frac{c\Delta T}{m}

e)

Q=mΔcTQ=m\Delta cT

22.

What is happening between D and E?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

Sublimation

23.

What is happening between B and C?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

Sublimation

24.

What state is the matter between C and D

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

e)

Not enough information to say

25.

Define Endothermic

a)

Energy is absorbed; ΔH is negative; Going from Liquid to Gas, and Gas to Liquid

b)

Energy is released; ΔH is negative; Going from Solid to Liquid, and Liquid to Gas

c)

Energy is released; ΔH is positive; Going from Solid to Liquid, and Liquid to Gas

d)

Energy is absorbed; ΔH is positive; Going from Solid to Liquid, and Liquid to Gas

26.

Define Exothermic

a)

Energy is absorbed; ΔH is negative; Going from Liquid to Gas, and Gas to Liquid

b)

Energy is released; ΔH is negative; Going from Solid to Liquid, and Liquid to Gas

c)

Energy is released; ΔH is negative; Going from Gas to Liquid, and Liquid to Solid

d)

Energy is absorbed; ΔH is positive; Going from Solid to Liquid, and Liquid to Gas

27.

Specific Heat is..

a)

the temperature initial minus temperature final

b)

the amount of heat/energy required to raise 1 gram of a substance by 1°C (or K) aka "C"

c)

the temperature final minus temperature initial

d)

the item in a system with given weight in grams

28.

What letter on the diagram represents a gas?

a)

A

b)

B

c)

C

d)

D

29.

What letter on the diagram represents a liquid?

a)

A

b)

B

c)

C

d)

D

30.

What letter on the diagram represents a solid?

a)

A

b)

B

c)

C

d)

D

31.

What letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

D

32.

What is the melting point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

33.

What is the boiling point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

34.

What would the state of this substance be at 0.5 ATM of pressure at a 100 degrees Celsius?

a)

Solid

b)

Liquid

c)

Gas

d)

X

35.

How many Joules of energy are required to make 50.0 grams of ice at 0 οC completely melt?

a)

334 J

b)

0 J

c)

33,400 J

d)

16,700 J

36.

The heat absorbed while a solid is melting is known as....

a)

heat of fusion

b)

heat of solid

c)

heat of liquid

d)

heat of vaporization

37.

Molarity is ...

a)

grams of solute/deciliters of solvent.

b)

grams of solute/liters of solution.

c)

moles of solute/liters of solution.

d)

moles of solute/milliliters of solvent.

38.

50 ml of a 1 M solution is diluted until the final volume is 80ml. How much water was added?

a)

50 ml

b)

1.3 ml

c)

30 ml

d)

130 ml

39.
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
40.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
41.

Calculate the Molarity in a solution containing 40.0 g of NaCl dissolved in 500.0 ml of H2O.

a)

0.08 M

b)

12.5 M

c)

1.37 M

d)

0.74 M

42.

How many mols of HCl are in 3 liters of 2.0M HCl solution?

a)

2.0

b)

1.5

c)

6.0

d)

0.66

43.

The mass % of aluminum in aluminum sulfate Al2(SO4)3 is:

a)

12.93%

b)

45.70%

c)

7.89%

d)

35.94%

e)

15.77%

44.

What is the mass percentage of Carbon in Carbon dioxide (CO2)?

a)

27.27%

b)

42.86%

c)

72.73%

d)

72.72%

45.
A saturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
46.
A supersaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
47.
An unsaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
48.
The dissolving medium in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
49.
The substance dissolved in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
50.
Which of the following word pairs correctly completes the sentence below?
_______ are corrosive substances characterized as having a strong smell, a sour taste, and a _______.
a)
Acids; pH less than 7
b)
Acids; pH greater than 7
c)
Bases; pH greater than 7
d)
Bases; pH less than 7
51.
If an acid is combined with a base of equal strength, the result will most likely be
a)
a neutral solution.
b)
a stronger acid.
c)
impossible to tell without testing the pH.
d)
a stronger base
52.
Which of the following is a base?
a)
orange juice
b)
water
c)
vinegar
d)
dishwashing detergent
53.
 Which of the following is an acid?
a)
shampoo
b)
baking soda
c)
orange juice
d)
water
54.
Which type of ion does a base produce when it is dissolved in water?
a)
oxide
b)
oxygen
c)
hydrogen
d)
hydroxide
55.
Which of the following is true about acids and bases?
a)
The lower the pH, the stronger the acid
b)
the higher the pH, the stronger the acid
c)
The lower the pH, the more neutral the acid
d)
The higher the pH, the weaker the base
56.
On the pH scale what numbers are bases?
a)
8-14
b)
0-7
c)
7
d)
1
57.
On the pH scale what numbers are acids?
a)
8-14
b)
0-7
c)
7
d)
1
58.
The pH scale measures...
a)
...the strength of an acid.
b)
...the strength of hydrogen ions.
c)
...the concentration of hydrogen ions.
d)
...the concentration of an acid
59.

Which type of ion does an acid produce when it is dissolved in water?

a)

oxide

b)

oxygen

c)

hydronium

d)

hydroxide

60.

What ions are there more of in acidic solutions?

a)

H+ (H3O+)

b)

OH-

61.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

62.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

63.

The pH of a solution is 8.43. What is the [H3O+]concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

64.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

65.

If the [OH-] of a solution is 2.7 x 10-4 M, the pOH of the solution is

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

66.
2NaClO3 (s) → 2NaCl (s) + 3O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
67.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
68.
N2 +  3H2 −->  2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
69.
How do I move from grams to moles
a)
multiply by molar mass
b)
divide by molar mass
c)
multiply by Avo number
d)
divided by Avo number
70.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
71.

What is the molar mass of Cl2?

a)

17 g/mol

b)

35.5 g/mo;

c)

71.0 g/mol

d)

89 g/mol

72.

What is the molar mass of UF6?

a)

101 g/mol

b)

238 g/mol

c)

257 g/mol

d)

352 g/mol

73.

Calculate the molar mass of KOH.

a)

28 g/mol

b)

56 g/mol

c)

84 g/mol

d)

112 g/mol

74.

How many moles are in 19.82 g Mg?

a)

1.23 mol Mg

b)

481.70 mol Mg

c)

1.00 mol Mg

d)

0.82 mol Mg

75.

What is the percent composition by mass of sulfur (S) in the compound MgSO4?

a)

20.22%

b)

19.85%

c)

26.64%

d)

28.64%

76.

Determine the mass of 4.20 moles of C6H12

a)

354 g

b)

84 g

c)

337 g

d)

421 g

77.

Use the given the chemical equation to answer the following question:

2C2H6 + O2 → 4CO2 + 6H2O


What does the number 4 represent for the formula unit 4CO2 ?

a)

The number 4 represents the coefficient, which is also equal to the number of grams of the formula unit above.

b)

The number 4 represents the subscript, which is also equal to the number of moles of the formula unit above.

c)

The number 4 represents the coefficient, which is also equal to the number of moles of the formula unit above.

d)

The number 4 represents the subscript, which is also equal to the number of grams of the formula unit above.

78.

What are the units for molar mass?

a)

grams

b)

amu

c)

grams/mole

d)

liters

79.
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
80.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
81.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
82.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
83.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
84.
When reacting Na with Cl2, we calculated that the theoretical yield should be 12.5 grams. Our actual yield was 13.0 grams. What is the percent yield?
a)
100%
b)
104%
c)
96%
d)
1.04
85.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
86.

What is the mass percentage of Oxygen in water (H2O)?

a)

11.11%

b)

88.89%

c)

33.33%

d)

66.67%

87.

Which of the following solutions is the most dilute?

a)

0.5M

b)

1M

c)

2M

d)

3M

88.

What is the pH of a solution with [H3O+] = 1 x 10-6 M?

a)

6

b)

-6

c)

1

d)

8

89.

Which process describes the change from a gas directly to a solid?

a)

Condensation

b)

Sublimation

c)

Deposition

d)

Melting

90.

What is the molar mass of NaCl?

a)

58.44 g/mol

b)

22.99 g/mol

c)

35.45 g/mol

d)

18.02 g/mol

91.

How many moles are present in 44.0 g of CO2?

a)

4.00 mol

b)

2.00 mol

c)

1.00 mol

d)

0.50 mol

92.

What is the volume of 2.0 moles of a gas at STP?

a)

22.4 L

b)

44.8 L

c)

2.0 L

d)

11.2 L

93.

Which type of intermolecular force is present in all molecules, regardless of their composition?

a)

Hydrogen bonding

b)

Ion-dipole forces

c)

Dipole-dipole interactions

d)

London dispersion forces

94.

What effect do strong intermolecular forces have on the boiling point of a substance?

a)

They lower the boiling point

b)

They raise the boiling point

c)

No effect on boiling point

d)

They make the boiling point unpredictable

95.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
96.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
97.
Does H2O have hydrogen bonding?
a)
yes
b)
no
98.
What information do we look for on the periodic table if we  want to examine intermolecular forces?
a)
atomic mass
b)
atomic number
c)
electronegativity
d)
ionization 
99.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

100.

Which of the following will increase the rate at which a solid dissolves in water?

a)

Using larger crystals

b)

Decreasing the temperature

c)

Stirring the solution

d)

Adding more solute

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