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Chemistry II Unit 5 Review

Total questions: 90

Worksheet time: 3hrs 37mins

Name
Class
Date
1.

As temperature rises ___________.

a)

an atom's kinetic energy decreases

b)

an atom's kinetic energy increases

c)

an atom's kinetic energy stays the same

2.

The more energy that particles have, the ___ they move.

a)

faster

b)

slower

3.

Charles' Law States...

a)

As Volume goes up temperature goes up 

b)

As Pressure goes down volume goes down 

c)

As Pressure goes up volume goes down

d)

As Pressure goes up temperature goes up

4.

Gas molecules are said to move

a)

with a set destination

b)

in random motion

c)

in attractive motion

d)

in a liquefiable motion

5.

Boyle's law : The pressure and volume of a gas show a _____ relationship.

a)

Inverse

b)

Direct

6.

Boyle's PV law : When _______ is held constant, the pressure and volume of a gas are ________ proportional

a)

temperature, equally

b)

temperature, inversely

c)

mass, equally

d)

mass, inversely

7.

Gas has no definite volume

a)

Fales

b)

True

8.

Which of the following can be considered a quality that gases display?

a)

Spread out to fill all available space

b)

Can be compressed

c)

Take the shape of their container

d)

All of these

9.

When Temperature of a gas increases, the Volume will ____________________

a)

Increase

b)

Decrease

c)

Stay the Same

10.

When Temperature of a gas increases, the Pressure will ____________________

a)

Increase

b)

Decrease

c)

Stay the Same

11.

When Volume of a gas increases, the Pressure will ______________

a)

Increase

b)

Decrease

c)

Stay the Same

12.

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

13.

What does the unit atmosphere, atm, measure?

a)

Pressure

b)

Temperature

c)

Volume

d)

Moles

14.

The pressure on a tank containing 0.3 moles of oxygen is 4.5 atm, and the temperature is 150 K. What is the volume of the gas?

(R = 0.0821)

a)

0.821 L

b)

8.21 L

c)

82.1 L

d)

821 L

15.

If you have 40 L of a gas at 6 atm, and 275K, how many moles will you have?

(R = 0.0821)

a)

10.6 mol

b)

0.1 mol

c)

150.5 mol

d)

81.2

16.

A sealed flask contains 1 mole of hydrogen and 3 moles of nitrogen at 20° C. If the total pressure is 400 torr, the partial pressure of the hydrogen is

a)

100 torr

b)

200 torr

c)

300 torr

d)

400 torr

17.

What does the unit Liters, L, measure?

a)

Volume

b)

Pressure

c)

Temperature

d)

Moles

18.

8 L of Helium gas are stored under a pressure of 3.3 atm. If there are 9.4 moles of Helium, what is the temperature of this sample of gas?

(R = 0.0821)

a)

34.2 K

b)

100 K

c)

273 K

d)

20.4 K

19.

Which of the following changes would cause a decrease in the Volume of a gas?

SELECT ALL THAT APPLY!!!

a)

Lowering the Temperature

b)

Increasing the Pressure

c)

Increasing the Temperature

d)

Lowering the Pressure

20.

Gas particles are in constant motion. They travel in straight lines, and they constantly bounce off the walls of any container that holds them.

What does this constant bombardment of particles against the walls of the container create?

a)

Pressure

b)

Density

c)

Temperature

d)

Magnetism

21.

A rubber tire holds 2.3 moles of CO2 at a temperature of 273 K. The volume of the tire is 8 L. What is the Pressure?

(R = 0.0821)

a)

6.4 atm

b)

412.4 atm

c)

43.5 atm

d)

3.1 atm

22.

Which of the following set of conditions would allow a gas to behave ideally?

(HINT: Remember that gases like to spread far apart! Which conditions would allow the molecules to easily spread apart?)

a)

High Temperature, Low Pressure

b)

High Temperature, High Pressure

c)

Low Temperature, High Pressure

d)

Low Temperature, Low Pressure

23.

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

24.

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

25.

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

26.

If a hairspray can is heated, what can be expected of the pressure of the gas inside the can?

a)

The pressure will increase

b)

The pressure will decrease

c)

The pressure will remain constant

d)

The pressure will equalize

27.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
28.
What is 50 °C in Kelvin?
a)
223
b)
323
c)
100
d)
50
29.
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
30.

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

31.

1. Which of the following correctly describes effusion?

a)

The movement of a gas into an area of higher pressure, always

b)

a. The movement of a gas into a vacuum (lower pressure area)

c)

a. The mixing of gases

d)

a. None of the above

32.

Which of the following correctly describes diffusion?

a)

The movement of gases into an area of higher pressure, always

b)

The movement of gases into a vacuum

c)

a. The mixing of gases

d)

a. Both (a) and (b)

33.

Which will travel faster: oxygen gas or helium gas?

a)

O2

b)

He

34.

Which travels faster? CO2 or Ar?

a)

CO2

b)

Ar

35.

Usuing Graham's Law: If you had 2 identical balloons filled with Nitrogen gas (N2) and Helium gas (He), which balloon will deflate the fastest?

a)

Helium balloon

b)

nitrogen balloon

c)

they will both deflate at the same rate

d)

the balloons will both pop

36.

a hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory

a)

Real Gas

b)

Ideal Gas

c)

Standard Gas

d)

Universal Gas

37.

1050 mmHg to atm

a)

1.38

b)

10.4

c)

798,000

d)

139.79

38.

250 C to K

a)

-23

b)

17

c)

487

d)

523

39.

Movement of molecules from an area of higher concentration to an area of lower concentration.

a)

Effusion

b)

Diffusion

c)

Ideal Gas

d)

Kinetic Molecular Theory

40.

Standard Temperature and Pressure

a)

1 atm 0 K

b)

1 atm 273 C

c)

760 mmHg 273 C

d)

760 mmHg 273 K

41.

2.3 atm to kPa

a)

0.023

b)

233

c)

44

d)

1748

42.

A process by which gas particles pass through a tiny opening

a)

Diffusion

b)

Effusion

c)

Kinetic Molecular

d)

Elastic

43.

Theory that all gases are composed of particles moving constantly in random directions

a)

Diffusion

b)

Effusion

c)

Kinetic Molecular

d)

Elastic

44.

91.3 kPa to mmHg

a)

0.90

b)

12.2

c)

69388

d)

685

45.

Which statement best describes how molecules move during DIFFUSION?

a)

They move from an area of HIGH concentration to an area of LOW concentration.

b)

They move from an area of LOW concentration to an area of HIGH concentration.

c)

They move closer together.

d)

None of the above

46.

IDENTIFY the gas law needed for the following calculation: Suppose you have a gas with 45.0 ml of volume and has a pressure of 760.mmHg. If the pressure is increased to 800mmHg and the temperature remains constant, what is the final volume?

a)

Charles'

b)

Boyle's

c)

Ideal Gas

d)

Avogadro's

47.

IDENTIFY the gas law needed for the following calculation: You have a gas that has volume of 2.5 liters and a temperature of 30 °C. What would be the final temperature if the gas has a volume of 4.5 liters?

a)

Avogadro's

b)

Boyle's

c)

Ideal Gas

d)

Charles'

48.

IDENTIFY the gas law needed for the following calculation: The only given information are number of moles and volumes.

a)

Ideal Gas

b)

Avogadro's

c)

Boyle's

d)

Charles'

49.

IDENTIFY the gas law needed for the following calculation: 5.00 L of a gas is known to contain 0.965 mol. If the amount of gas is increased to 1.80 mol, what new volume will result (at an unchanged temperature and pressure)?

a)

Ideal Gas

b)

Charles'

c)

Boyle's

d)

Avogadro's

50.

IDENTIFY the gas law needed for the following calculation: The initial volume of a gas is 300.0 mL and has a pressure of 99.0 kPa . If the final pressure is increased to 188 kPa, what will be the final volume in mL?

a)

Charles'

b)

Ideal Gas

c)

Boyle's

d)

Avogadro's

51.

IDENTIFY the gas law needed for the following calculation: A sample of gas has a volume of 12.3 mL and a temperature of 22.5 oC. what will be the new volume if the gas is heated to 85 oC?

a)

Avogadro's

b)

Charles'

c)

Boyle's

d)

Ideal Gas

52.

IDENTIFY the gas law needed for the following calculation: The information provided to solve the problem is temperatures and volumes.

a)

Ideal Gas

b)

Avogadro's

c)

Boyle's

d)

Charles'

53.

IDENTIFY the gas law needed for the following calculation: The temperature inside my refrigerator is about 4 oC. If I place a balloon in my fridge that initially has a temperature of 22 oC and a volume of 0.5 liters, what will be the final volume of the balloon when it is fully cooled by my refrigerator?

a)

Charles'

b)

Boyle's

c)

Avogadro's

d)

Ideal Gas

54.

IDENTIFY the gas law needed for the following calculation: A sample of gas occupies 2.00 L with 5.00 moles present. What would happen to the volume if the number of moles is increased to 10.0 moles?

a)

Boyle's

b)

Avogadro's

c)

Charles'

d)

Ideal Gas

55.

IDENTIFY the gas law needed for the following calculation: What happened to the number of moles in a sample that originally occupied 500 ml with 2.5 moles and then occupied 750 ml?

a)

Charles'

b)

Boyle's

c)

Avogadro's

d)

Ideal Gas

56.

IDENTIFY the gas law needed for the following calculation: The information provided are pressures and volumes.

a)

Boyle's

b)

Charles'

c)

Avogadro's

d)

Ideal Gas

57.

IDENTIFY the gas law needed for the following calculation: A balloon had an initial volume of 75L and a temperature of 25 oC. What would the final temperature need to be in order for the balloon to have a final volume of 100L at the same pressure?

a)

Boyle's

b)

Ideal Gas

c)

Charles'

d)

Avogadro's

58.

V1/n1 = V2/n2 is ___________ Law formula

a)

Ideal Gas

b)

Charles'

c)

Boyle's

d)

Avogadro's

59.

IDENTIFY the gas law needed for the following calculation: A gas was cooled to 342 K in order to decrease the volume to 85 liters. If the initial volume was 130 liters of gas in a piston, what was the initial temperature?

a)

Boyle's

b)

Ideal Gas

c)

Charles'

d)

Avogadro's

60.

IDENTIFY the gas law needed for the following calculation: An unknown gas initially has a volume of 10 ml and a pressure of 2.5 atm. What is the volume if the pressure is increased to 4 atm?

a)

Boyle's

b)

Charles'

c)

Avogadro's

d)

Ideal Gas

61.

P1/V2 = P2/V1 is _________ Law

a)

Ideal

b)

Charles'

c)

Boyle's

d)

Avogadro's

62.

PT = P1 + P2 + P3 + ..... is ___________________

a)

Avogadro's Law

b)

the Ideal Gas Law

c)

Charles' Law

d)

Dalton's Law

63.

The law that uses only pressures is-

a)

Dalton's Law of Partial Pressures

b)

Avogadro's Law

c)

Ideal Gas Law

d)

Boyle's Law

64.

V1/T1 = V2/T2 is-

a)

Ideal Gas Law

b)

Charles' Law

c)

Boyle's Law

d)

Avogadro's Law

65.

Which formula contains only one variable:

a)

Boyle's Law

b)

Charles' Law

c)

Avogadro's Law

d)

Dalton's Law of Partial Pressures

66.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the rate.
67.

For a reaction 2A + B --> 2C, with the rate equation:

Rate = k [A]2 [B]

a)

The order with respect to A is 1 and the order overall is 1

b)

The order with respect to A is 2 and the order overall is 2

c)

The order with respect to A is 2 and the order overall is 3

d)

The order with respect to B is 2 and the order overall is 3

e)

The order with respect to B is 2 and the order overall is 2

68.
What is the rate exponent for A?
a)
0
b)
1
c)
2
69.
What is the rate exponent for B?
a)
0
b)
1
c)
2
70.
Rate of chemical reaction means
a)
amount of product formed
b)
speed of reaction
c)
concentration of reacting particles
d)
combining reactants with products
71.
All changes in the state of matter of a substance requires
a)
vibration
b)
water
c)
permission
d)
energy
72.
Change from Liquid to Solid is call......
a)
fusion
b)
Freezing
c)
sublimation
d)
evaporation
73.

Temperature is a measure of the average _____________ energy of the particles of a substance.

a)

potential

b)

kinetic

c)

gravitational

d)

heat

74.

Which letter represents particles in solid form?

a)

A

b)

B

c)

C

d)

D

e)

E

75.

Between which points is the temperature of the substance remaining constant? (Diagram F)

a)

A-B only.

b)

A-B, C-D, E-F

c)

B-C only.

d)

B-C, D-E

76.

Predict the products for the this reaction:

Mg + CuCl2 -->

a)

MgCl2 + Cu

b)

MgCl + Cu

c)

MgCu + Cl2

d)

CuMg + Cl2

77.
The reaction below is an example of?
AgNO3 + NaCl → AgCl + NaNO3
a)
Single Replacement
b)
Double Replacement
c)
Decomposition
d)
Combustion
78.
What type of reaction is illustrated below?
2HI --> H2  +  I2
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
79.

Balance this equation.

_CF4 + _Br2 -- _CBr4 + _F2

a)

2,1,2,1

b)

1,2,2,1

c)

1,2,1,2

d)

2,2,2,2

80.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
81.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (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
82.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
83.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
84.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
85.

Balance this equation

_Al +_HCl --> _H2 +_AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

86.
Balance this equation:
P4+O2  -->  P2O3
a)
3 P4+ O2 --> 2 P2O3
b)
 P4+ O2 --> 2 P2O3
c)
 P4+ 3 O2 --> 2 P2O3
d)
 P4+ 2 O2 --> 3 P2O3
87.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
88.
Exothermic reactions...
a)
Absorb energy
b)
Release energy
c)
Release Color
d)
Absorb Color
89.

Which conversion factor should be used for the following question - How many molecules are there in 4.00 moles of glucose, C6H12O6? 

a)
1 mole = 78.12 g
b)
1 mole = 22.4 L 
c)
1 mol = 6.02x 1023 particles 
d)
more than one
90.

Which conversion factor should be used for the following question - How many liters are there in 1.00 moles of carbon dioxide? 

a)
1 mole = 78.12 g
b)
1 mole = 22.4 L 
c)
1 mol = 6.02x 1023 particles 
d)
more than one

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