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U3P1 Review

Total questions: 98

Worksheet time: 7hrs 51mins

Name
Class
Date
1.
QT 1 - Which of the following is true regarding state functions?
a)
State functions only concentrate on the change between the beginning and end
b)
State functions only care for the path taken to achieve the results
c)
State functions care for the begining, end, and the path taken to achieve the results
d)
State functions are unnecesary and are not interested in any parts of its procedure
2.
QT 1 - Which of the following is an intensive property?
a)
Pressure
b)
Temperature
c)
Volume
d)
Moles
3.
QT 8 - What is the volume of the gas, CO2, when there are 132 Grams, a pressure of 5 atm, and a temperature of 27 Degrees Celcius?
a)
22.4 Liters
b)
14.7 Liters
c)
34.1 Liters
d)
5.8 Liters
4.
QT 8 - At STP, how many moles are in 33.6 Liters of SF6?
a)
1.5 Moles
b)
2.9 Moles
c)
3.1 Moles
d)
4.7 Moles
5.

QT 8 - What is the mass of HCl if you have 44 liters at STP?

a)

21.8 grams

b)

10 grams

c)

72 grams

d)

36 grams

6.

QT 3-Maxwell Distributions - If a system has a low temperature, what will the distribution look like?

a)
Tall and Narrow
b)
Broad and short
c)
Right in the middle
d)
Tall and Broad
7.

QT 6 - What percentage of the pressure at STP will the hydrogen in CH4 be?

a)
0.8
b)
0.2
c)
0.75
d)
0.25
8.

QT 2 - Kinetic Molecular Theory - According to the Kinetic Molecular Theory, which of the following statements is incorrect?

a)
Gas molecules have non elastic collisions.
b)
Gases are simple, hard spheres.
c)

Mass is inverse and square to velocity.

d)
The larger a gas is, the slower it will move.
9.

QT 2. Kinetic Molecular Theory - If the temperature doubled, the kinetic energy of the gas molecules would-

a)
Increase
b)
Decrease
c)
Stay the same
d)
None of the above
10.

QT 2. Kinetic Molecular Theory - What does v stand for in the formula: v= (KT/m)^2?

a)
Volume
b)
Velocity
c)
Vacuum
d)
Valency
11.
QT 4 - What two gases achieve a ratio of gas velocities equal to a 5:1 ratio?
a)
He and Ne
b)
O2 and H2
c)
He and O2
d)
HBr and He
12.
QT 4 - What conditions are best for diffusion/ effusion?
a)

high temperature and large particle size

b)

low temp and large particle size

c)

high temp and small particle size

d)

low temp and small particle size

13.
QT 4 - What is the expected ratio of gas velocities for He compared to H2?
a)
He is 4 times faster than H2
b)
He is 2 times faster than H2
c)
H2 is 4 times faster than He
d)
H2 is 2 times faster than He
14.

QT 9 - Which temperature change would cause a sample of an ideal gas to double in volume while the pressure is held constant?

a)
200 K to 400 K
b)
800 K to 600 K
c)
400 K to 200 K
d)
600 K to 800 K
15.

QT 9 - 2 H2+ O2---> 2 H2O; Three atm of hydrogen gas react with one atm oxygen gas in a closed container with rigid walls. What happened to the pressure in the vessel?

a)
Presure decreased
b)
no change in pressure
c)
No way to tell
d)
Pressure increased
16.
QT 11 - Which of the following is the most ideal gas?
a)
HCl
b)
Kr
c)
CO2
d)
Ne
17.

QT 11 - Which of the following is the most ideal gas?

a)

CH4

b)

HCl

c)

O2

d)

NaCl

18.

QT 12 - What is the correct way to order strength of covalent bonds in intramolecular forces?

a)
Covalent double bond < Covalent triple bond < Covalent single bond
b)
Covalent triple bond < Covalent double bond < Covalent single bond
c)
Covalent single bond < Covalent double bond < Covalent triple bond
d)
Covalent double bond < Covalent single bond < Covalent triple bond
19.
QT 12 - What is the correct way to order ionic bonds on the number line? *Hint: Similar to covalent bonds
a)
Single charge < double charge < triple charge
b)
Triple charge < double charge < single charge
c)
Single charge > double charge > triple charge
d)
Double charge < triple charge < single charge
20.
QT 9 - C3H8 + 5O2 → 3CO2 + 4H2O; If we combust 3 liters of propane in excess oxygen, how many liters of CO2 and H2O did we make?
a)
9
b)
12
c)
21
d)
24
21.

U0-7. Which problem is balanced?

a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
22.

U0-7. KNO3 --> KNO2 + O2 What coefficients are needed to balance the reaction?

a)
2, 2, 1
b)
2, 3, 2
c)
1, 2, 2
d)
1, 3, 1
23.

U0-17. Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.

a)
AlCl3
b)
Cl2
c)
Al
24.

QT U0-18. What is the excess reactant if 8 moles of NH3 react with 18 moles of NO and how much is left over?

4 NH3 + 6 NO --> 5 N2 + 6 H2O

a)

NH3, 12 moles

b)

NO, 6 moles

c)

NH3, 6 moles

d)

NO, 12 moles

25.

QT 12. Which of the following is the weakest?

a)

Intramolecular Forces- Double Bonds

b)

Intramolecular Forces- Single Bonds

c)

Intermolecular Forces- Polar Molecules

d)

Intermolecular Forces- NonPolar Molecules

26.

QT. 10 Under which conditions of temperature and pressure does carbon dioxide behave most like an ideal gas?

a)

Low temperature and low pressure

b)

Low temperature and high pressure

c)

High temperature and low pressure

d)

High temperature and high pressure

27.

QT 10. Which of the following gases would have the largest a and b correction factors respectively:

C3H8 , H2O , CH4 , N2

a)

C3H8 , H2O

b)

H2O , CH4

c)

H2O , C3H8

d)

H2O , N2

28.

QT 10. Which of the following are true?

a)

The b correction factor adjusts pressure based on how "sticky" the molecule is

b)

The a correction factor adjusts pressure based on how "sticky" the molecule is

c)

The a correction factor adjusts volume based on the size of the molecule

d)

The b correction factor adjusts volume based on the size of the molecule

29.

A gas that has a pressure of 2 atm and a volume of 10 L.  What equation would you use to calculate the new volume if the pressure was changed to 1 atm?

a)
P1/T1 = P2/T2
b)
P1V1 = P2V2
c)
V1/n1 = V2/n2
d)
PV = nRT
30.

QT 5. You have a gas that has a pressure of 2 ATM and a volume of 10L.  What would be the new volume if the pressure was changed to 1 ATM?

a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
31.

QT 5. In order to convert to Kelvin, you add ______ to the Celsius measurement.

a)
372
b)
273
c)
237
d)
732
32.

QT 5. If 200 mL of a gas at 27°C is cooled to -33°C at a constant pressure, the volume will be

a)
250 mL
b)
204 mL
c)
196 mL
d)
160 mL
33.

The diagram shows the Maxwell−Boltzmann distribution of molecular energies in a gas at two different temperatures.


Which letter represents the most probable energy of the molecules at the higher temperature?

a)

A

b)

B

c)

C

d)

D

34.

The question below is about the Maxwell–Boltzmann distribution shown for a sample of a gas, X, at two different temperatures.


Which letter shows the mean energy of the molecules at the higher temperature?

a)

P

b)

Q

c)

R

d)

S

35.

This question is about the Maxwell–Boltzmann distribution of molecular energies in a sample of a gas shown in the figure below.


What does the area under the curve represent?

a)

The total energy of the particles.

b)

The total number of particles.

c)

The number of particles that can react with each other.

d)

The total number of particles that have activation energy.

36.

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

37.

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

a)

Inverse

b)

Direct

38.

Whose law states that as pressure goes up, volume goes down?

a)

Mazias

b)

Boyle

c)

Charles

d)

Aglow

39.

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

40.

You leave a soccer ball outside in the winter. Will the ball end up flatter than it was before?

a)

Only if it's REALLY cold

b)

No

c)

Only if it has a leak

d)

Yes

41.

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

42.

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

a)

faster

b)

slower

43.

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

44.

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

45.

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

46.

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

47.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
48.
What is 50 °C in Kelvin?
a)
223
b)
323
c)
100
d)
50
49.
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
50.

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

51.

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.

52.

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

53.

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

54.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
55.

What describes the motion of a Gas Molecule?

a)

Molecules are far apart

b)

Move in constant, random motion

c)

It will travel in a straight path

d)

All of the above

56.
Boyle's law :  The pressure and volume of a gas show a _____ relationship. 
a)
Inverse 
b)
Direct 
57.
How many nitrogen atoms does NH3 have?
a)
1
b)
2
c)
3
d)
4
58.
Bob puts 200 grams of ice into a pitcher with 900 grams of water. He gets distracted and comes back later to find that the ice has melted in the water. How many grams of water does Bob now have in the pitcher?
a)
200 g
b)
700 g
c)
1,100 g
59.

A gas that has a pressure of 2 atm and a volume of 10 L. What would be the new volume if the pressure was changed to 4 atm?

a)

2 L

b)

4 L

c)

8 L

d)

5 L

60.
What will happen to the volume of a gas if the pressure increases, with constant temperature ?
a)
Increase
b)
Decrease
c)
Nothing
d)
Explosion!
61.

All of the following are temperature units except ______

a)

atm

b)

Kelvin

c)

Celsius

d)

Farenheit

62.

.001 L

a)

1ml

b)

10 ml

c)

100 ml

d)

.01 ml

63.
The rate of effusion is _______________ proportional to the square root of its' molar mass. 
a)
Directly
b)
Inversely 
64.
Lighter gases have a ________________ rate of effusion.
a)
faster 
b)
slower
c)
rate of effusion does not depend on mass.
65.
Which of the following would have a faster rate of effusion: 15g of Kr or 15g of N2?
a)
Kyrpton
b)
Nitrogen
c)
Both would have the same rate of effusion
66.

why would O2 effuse faster than CO2 in the same room

a)

because O2 has more energy

b)

because CO2 has a greater molar mass

c)

because oxygen has a higher temperature

d)

they will effuse the same because the temperature is fixed

67.
Use Graham’s Law to calculate fast O2 gas will effuse compared to Cl2. 
a)
O2 effuses 1.5x faster than Cl2
b)
O2 effuses 0.11x as fast as Cl2
c)
O2 effuses 1.1x faster than Cl2
d)
O2 effuses 0.15x as fast as Cl2
68.

How much faster will He(g) travel than O2(g)?

a)

4 times faster

b)

2.8 times faster

c)

0.35 times faster

d)

0.125 times faster

69.

Which of the following is the equation needed to calculate the kinetic energy, KE, of a moving particle?

a)

KE = 1/2 mv2

b)

KE = 2mv

c)

KE = mv

d)

KE = 1/2 m2v

70.

If a gas has the same temperature throughout, which gas molecule has the highest average velocity?

a)

O2

b)

H2O

c)

H2

d)

Xe

71.

Which condition is necessary for most gases to behave nearly ideally?

a)

high pressure

b)

high temperature

c)

low compressibility

d)

low expansion

72.

Which gas deviates the most from ideal behavior?

a)

CH4

b)

H2O

c)

Cl2

d)

He

73.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

74.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

75.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

76.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

77.

In a polar covalent bond, which atom will have a partial positive charge? (choose 2 correct answers)

a)

The atom that attracts fewer electrons

b)

The atom with the greater electronegitivity

c)

The atom that attracts more electrons

d)

The atom with the lower electronegativity

78.

What must the difference in electronegativity between two atoms be in order for the bond between them to be polar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

79.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

80.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

81.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

82.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

83.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

84.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

85.

When you have C-H, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

86.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
87.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
88.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
89.

True or False


Attractions between polar molecules are Weaker than attractions between nonpolar molecules.

a)

True

b)

False

90.
Which molecule contains bonds with a GREATER polarity?
a)
HCl
b)
CCl4
91.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

92.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

93.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

94.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

95.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

96.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
97.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
98.
Which formula represents a polar molecule?
a)
H2
b)
H2O
c)
CO2
d)
CCl4

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