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Exam 3

Total questions: 107

Worksheet time: 5hrs 5mins

Name
Class
Date
1.

Which force is only found between polar covalent molecules?

a)

Ionic bond

b)

Dipole Dipole

c)

London Dispersion Force

d)

Covalent bond

2.

In ionic solids, what holds the ions together?

a)

Hydrogen Bonding

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

3.

In this force, electron movement cause a slight charge at a single instant. This charge is temporary.

a)

Hydrogen bonding

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

4.

Which is not a bond, but is an intermolecular force?

a)

Covalent Bond

b)

Ionic Bond

c)

Hydrogen Bond

d)

These are all bonds

5.

All polar covalent molecule samples contain:

(Check all that apply)

a)

Hydrogen bonds

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

6.

Samples of H2O, NH3, and HF all contain:

(Check all that apply)

a)

Hydrogen Bonds

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

7.

Nonpolar molecule samples all contain

(Check all that apply)

a)

Hydrogen Bonding

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

8.
Does HCl have hydrogen bonding?
a)
yes
b)
no
9.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
10.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

11.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
12.
Does HF have hydrogen bonding?
a)
yes
b)
no
13.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

14.
The strength of temporary dipoles:
a)
increases with the size of molecules
b)
is greater than intremolecular forces
c)
is the strongest intermolecular force
15.
If a liquid has high viscosity, it probably has:
a)
strong IMF
b)
weak IMF
16.

Which compound in liquid form will have the highest vapor pressure?

a)

CH4

b)

CH3CH3

c)

CH3COCH3

d)

CH3CH2OH

17.
Which of these typically increases when intermolecular forces increase?
a)
Boiling Point
b)
Melting Point
c)
Viscosity
d)
All of these
18.
A substance capable of hydrogen bonding has a ___________ boiling point than a similar substance that doesn't hydrogen bond.
a)
higher
b)
lower
19.
Which of these typically decreases when IMF's increase?
a)
boiling point
b)
melting point
c)
all of these
d)
vapor pressure
20.
If a liquid has high viscosity, it probably has:
a)
strong IMF
b)
weak IMF
21.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
22.

Which noble gas should have the highest boiling point? (Hint: Think about how size affects IMFs)

a)

He

b)

Ne

c)

Kr

d)

Xe

23.

Does NH3 or PH3 have a higher boiling point?

(Hint: identify the types of IMF's present for each)

a)

NH3 because it has the strongest IMF's

b)

PH3 because it has the strongest IMF's

c)

NH3 because it has the weakest IMF's

d)

PH3 because it has the weakest IMF's

24.

Has a set shape and a set volume

a)

solid

b)

liquid

c)

gas

d)

plasma

25.

Has a set volume but no set shape

a)

solid

b)

liquid

c)

gas

d)

plasma

26.

Has no set volume and no set shape

a)

solid

b)

liquid

c)

gas

d)

plasma

27.

These demonstrate particles of a...

a)

solid

b)

liquid

c)

gas

d)

plasma

28.

These demonstrate particles of a...

a)

solid

b)

liquid

c)

gas

d)

plasma

29.

These demonstrate particles of a...

a)

solid

b)

liquid

c)

gas

d)

plasma

30.

Evaporation is the change in state of a

a)

gas to a liquid

b)

gas to a solid

c)

solid to a liquid

d)

liquid to a gas

31.

The boiling point of a substance is the temperature at which it changes from

a)

a liquid to a gas

b)

a liquid to a solid

c)

a gas to a solid

d)

a solid to a liquid

32.

Transition from a liquid to a gas

a)

Condensation

b)

Freezing

c)

Evaporation

d)

Melting

33.

Gas condenses to a liquid

a)

Evaporation

b)

Melting

c)

Freezing

d)

Condensation

34.

Three containers with the same amount of the same material are shown below. Which container has the substance with the highest amount of energy?

a)

The container on the left

b)

The middle container

c)

The container on the right

d)

All have an equal amount of energy

35.

Three containers with the same amount of the same material are shown below. Which container has the substance with the lowest amount of energy?

a)

The container on the left

b)

The middle container

c)

The container on the right

d)

All have an equal amount of energy

36.

Transition from a solid to a liquid

a)

Condensation

b)

Melting

c)

Freezing

d)

Evaporation

37.

Transition from a liquid to a solid

a)

Freezing

b)

Sublimation

c)

Melting

d)

Evaporation

38.

Change of a solid directly into a gas

a)

Deposition

b)

Melting

c)

Sublimation

d)

Freezing

39.

Change of a gas directly into a solid

a)

Sublimation

b)

Condensation

c)

Evaporation

d)

Deposition

40.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
41.

In an endothermic reaction, heat is ...

a)

taken in

b)

given out

42.

(You may use scratch paper and a calculator)

How much energy is required to change 30 grams of water from 20 οC to 90 οC?


The specific heat of water = 1 cal/goC

a)

70 J

b)

2100 J

c)

2700 J

d)

600 J

43.

In this Equation "q" stands for

a)

Mass of Fuel

b)

energy absorbed or released by the substance

c)

change in temperature

d)

mass of substance being heated

e)

amount of energy needed to raise the temperature for that substance

44.

A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat of iron.

a)

0.46 J/goC

b)

2,567,446.875 J/goC

c)

1.654 J/goC

45.

How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22.0°C to 55.0°C, if the specific heat of aluminum is 0.903 J/g°C?

a)

298 Joules

b)

297 J/g°C

c)

0.003 Joules

d)

0.003 J/g°C

46.

The specific heat(c) of copper is 0.38 J/g °C. What is the temperature change(∆t) when 100.0 Joules of heat(Q) is added to 20.0 grams?

a)

13 °C

b)

15 °C

c)

20 °C

47.

If you add 50 J of energy to a piece of iron, and the temperature rises (changes) by 25.0°C, what is the mass of the iron? (Iron has a specific heat of 0.10 J/g°C)

a)

25 g

b)

30 g

c)

20 g

d)

50 g

48.

Which equation should you use:

How much heat is required to melt 10.0 grams of H2O?

a)

Q =mΔHvap

b)

Q =mCΔT

c)

Q =m(-ΔHfus)

d)

Q =mΔHfus

49.
What does "#4" represent on the graph? 
a)
melting 
b)
liquid phase
c)
boiling
d)
gas phase
50.
What does "#2" represent on the graph? 
a)
solid phase
b)
melting
c)
liquid phase
d)
boiling
51.
What does "#5" represent on the graph? 
a)
solid phase 
b)
melting
c)
boiling
d)
gas phase
52.
What does "#3" represent on the graph? 
a)
melting
b)
liquid phase
c)
boiling
d)
gas phase
53.

How much energy must be removed to make 150.0 gram s of water at 0.0 °\degree  C freeze? ( \Delta  Hfus = 6.00kJ/mol)

a)

900. J

b)

49.9 J

c)

900. kJ

d)

49.9 kJ

54.

How much energy would you need to add to make 250 grams of water boil? (ΔHvap= 40.7 kJ/mol)

a)

560 kJ

b)

560 J

c)

10,000 kJ

d)

10,000 J

55.

During A to B what phase of matter is the substance?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

56.

From B to C, a solid is changing to a liquid. Is heat being added or taken away during this time?

a)

Added

b)

Taken away

57.

From C to D, what phase of matter is the substance?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

58.

From D to E, a liquid is being changed to a gas. Is heat being added or taken away during this time?

a)

Added

b)

Taken away

59.

From E to F, what phase of matter is the substance?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

60.

Where is vaporization occurring?

a)

A

b)

B

c)

D

d)

E

61.
What is the new volume of the gas if the pressure on 350 L of oxygen at 720 mm Hg is decreased to 600 mm Hg?
a)
420 L
b)
29.16 L
c)
4200.0 L
d)
291.6 L
62.
A gas occupies 4.98 L at 2.6 atm of pressure. What volume does it occupy at 1.8 atm pressure?
a)
12.9 L
b)
0.72 L
c)
7.2 L
d)
3.44 L
63.
A gas at a volume of 4 liters is at a pressure of 2 atm. The volume is changed to 16 Liters, what must the new pressure be?
a)
2 atm
b)
12 atm
c)
10 atm
d)
0.5 atm
64.

(Charles Law) There are 65 liters of helium in a balloon at 35 K. If the temperature of the balloon is increased to 40 K, what will the new volume of the balloon be?

a)

40 L

b)

70 L

c)

74.3 L

d)

75.9 L

65.

A sample of nitrogen occupies a volume of 250 mL at 25oC. What volume will it occupy at 95oC?

a)

308.70 mL

b)

456.1 mL

c)

308.70oC

d)

456.1oC

66.

Oxygen gas is at a temperature of 40oC when it occupies a volume of 2.3 liters. To what temperature should it be raised to occupy a volume of 6.5 liters?

a)

611.84oC

b)

611.84 K

c)

880.33 K

d)

880.33oC

67.

Hydrogen gas was cooled from 150oC to 50oC. Its new volume is 75 mL. What was its original volume?

a)

98 mL

b)

98 K

c)

98oC

d)

98 L

68.

A rigid plastic container holds 1.00 L methane gas at 0.9 atm pressure when the temperature is 22.0°C. How much more pressure will the gas exert if the temperature is raised to 44.6°C?

a)

0.97 atm

b)

1.82 atm

c)

0.97oC

d)

1.82oC

69.

If a gas sample has a pressure of 30.7 kPa at 0.00°C, by how much does the temperature have to decrease to lower the pressure to 28.4 kPa?

a)

33.89 oC

b)

-20.46 oC

c)

597 oC

d)

-4.25 oC

70.
How much volume does 3 moles of chlorine gas occupy at STP?
a)
250 L
b)
213 L
c)
106.5 L
d)
67.2 L
71.
Calculate the partial pressure of H2 at 20oC when the vapor pressure of water is 17.5torr. The total pressure of the gases is 750torr.
a)
767.5torr
b)
732torr
c)
42.86torr
72.
A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?
a)
234 mmHg
b)
1.37 mmHg
c)
2.64 mmHg
d)
1, 494 mmHg
73.

The total pressure of a mix of gases is...?

a)

Greater than the sum of the pressures of the mix of gases

b)

The sum of the partial pressures of the individual gases

c)

The masses of all the gases combined

d)

Equal to the most pressurized gas

74.
Solutions are composed of __________ .
a)
salts and solutes
b)
solvents and salts
c)
solutes and alloys
d)
solutes and solvents
75.
If we are making Kool-aid with sugar, Kool-aid powder, and water, which part is the solvent?
a)
water
b)
powder
c)
sugar
d)
powder and sugar
76.
In this mixture, which of the following will be the solute?
a)
The water in the glass
b)
The glass that holds the final mixture
c)
The solution containing both powder and water
d)
The powder on the spoon
77.

. “Like dissolves like” is a rule that can be used to predict a solute’s solubility in a solvent. Which choice agrees with this statement?

a)

CH3CH2CH2CH2CH2CH3 should dissolve in a polar solvent.

b)

CH3CH2CH2CH2CH2CH3 should not dissolve in gasoline

c)

CH3CH2OH should dissolve in water

d)

MgCl2(s) should not dissolve in polar solvent.

78.

All of the following substances will dissolve in water EXCEPT:

a)

C6H6

b)

Ca(NO3)2

c)

AlCl3

d)

CH3CH2OH

79.

Sodium chloride is LEAST soluble in which of the following liquids?

a)

CH3OH

b)

Water

c)

CCl4

d)

HF

80.

Which one of the following substances would be the most soluble in CCl4?

a)

NaCl

b)

H2O

c)

NH3

d)

C10H22

81.

Which of the following substances is more likely to dissolve in benzene (C6H6)

a)

NaCl

b)

NH3

c)

CCl4

d)

CH3CH2OH

82.
a solute whose water solution conducts electricity is called a(n)
a)
nonconductor
b)
electrolyte
c)
nonelectrolyte
d)
aqueous solution
83.

What is the percent composition of oxygen in MgO?

a)

20%

b)

40%

c)

50%

d)

60%

84.

What is the percent composition of sodium in NaCl?

a)

39%

b)

61%

c)

35%

d)

65%

85.
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
86.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

87.

You want to make 60 ml of a 20% NaCl solution. (NaCl (table salt) is measured using a balance.)

How much NaCl do you need and how do you make this solution? write number and units only

(a)  

88.

If you put 40.g of sugar into a final volume of 1.0 L of dH2O (distilled), what percent sugar is your solution? (number and unit only)

(a)  

89.

What mass of water should be added to 22.0 g of KCl to make 5.50% by mass solution?

a)

400 g

b)

40 g

c)

0.25 g

d)

25 g

90.

How many grams of NaNO3 are needed to prepare 100 g of 15.0 % by mass NaNO3 solution? (MM = 85 g/mol)

a)

15 g

b)

1275 g

c)

12.75 g

d)

150 g

91.

What is the molarity of 0.068 mol of NaCl in 3.8 L of solution?

a)

0.018 M

b)

0.0011 M

c)

1.052 M

d)

0.062 M

92.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
93.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
94.
How many L are required to make 3.5 M hydrochloric acid using 1.1 moles? 
a)
3.18 L
b)
0.31 L
c)
3.85 L
d)
4.6 L
95.
If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?
a)
20.9 mol
b)
0.021 mol
c)
0.02 mol
d)
0.0209 mol
96.

How many mL of stock solution of 2M NaCl do you need to prepare 100 mL of 0.150M NaCl?

a)

7.5 mL

b)

15 mL

c)

1333 mL

d)

200 mL

97.

How many mL of 1.0M KBr solution would you need to prepare 250 mL of a 0.2M dilution?

a)

175 mL

b)

250 mL

c)

50 mL

d)

5 mL

98.

Which of the following is the Dilution Formula?

a)

V1M1 = V2M2

b)

M = m/V

c)

V = mT

d)

PV = nRT

99.

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

100.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
101.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
102.

Determine the freezing point of a 0.08 m solution dissolved in water (0°C freezing point and Kf = 1.86°C)

a)

-0.15 °C

b)

0.004 °C

c)

1 °C

d)

-11 °C

103.
What is the freezing point of a 1.5 m solution of sucrose in water? (Kf = 1.86°C/m)
a)
-2.8°C
b)
-1.2°C
c)
-0.81°C
d)
0.81°C
104.
Balancing this reaction: ____ CH4 + ____ O2 ---> ____ CO2 + ____ H2O
a)
2,1,3,1
b)
1,2,1,2
c)
1,2,2,1
d)
2,1,1,2
105.
Balance this reaction: ____ NaF + ____ Br2 ---> ____ NaBr + ____ F2
a)
3,1,2,1
b)
1,2,3,4
c)
2,1,2,1
d)
1,2,1,2
106.
Balance this equation:
Al2O3 -> Al + O2 
a)
2Al2O3 -> 2Al + 3O2 
b)
2Al2O3 -> 4Al + 3O2 
c)
3Al2O3 -> 2Al + O2 
d)
2Al2O3 -> 3Al + 2O2 
107.
Balance this equation
_Zn+_HCl-->_ZnCl2 +_H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1

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