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Unit 3A Review-IMF and Ideal Gas

Total questions: 65

Worksheet time: 56mins

Name
Class
Date
1.

Determine the number of moles in a container of gas at 1 atm with a volume of 99.2 L and a temperature of 100K.

a)

12 mol

b)

120 mol

c)

10 mol

d)

100 mol

2.
If the pressure exerted by a gas at 298 K in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?
a)

6.85 mol

b)

0.007 mol

c)

6.9 mol

d)

0.0069 mol

3.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
4.
How do gas molecules move? 
a)
in an orderly fashion 
b)
constantly and randomly
c)
in straight line paths
d)
in a circular motion
5.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
6.
When Volume increases then Pressure must...
a)
Increase
b)
Decrease
7.
What type of relationship to pressure and volume have?
a)
direct
b)
inverse
c)
no relationship
d)
I don't know
8.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
9.
Gases have...
a)
A definite shape and volume
b)
A definite shape but no definite volume
c)
No definite shape but a definite volume
d)
No definite shape or volume
10.
What is the variable for this number 22.4 L
a)
P
b)
T
c)
n
d)
V
11.
What is the variable for this number 32oC
a)
P
b)
T
c)
n
d)
V
12.
What is the variable for this number 9.10 atm
a)
P
b)
T
c)
n
d)
V
13.
What is the variable for this number 122 K
a)
P
b)
T
c)
n
d)
V
14.
What is the variable for this number 1.5 mol
a)
P
b)
T
c)
n
d)
V
15.
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
16.
Determine the Kelvin 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)

310. K 

17.
Determine the Celsius temperature of 2.49 moles of gas contained in a 1.00-L vessel at a pressure of 143 kPa. 
a)
-266 degrees C
b)
-622 degrees C
c)
622 degrees C 
d)
266 degrees C
18.
What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 320 K?
PV=nRT
a)

14 atm

b)

16.53 atm

c)

14.19 atm

d)

22.54 atm

19.
As number of moles goes up, volume 
a)
goes down.
b)
goes up.
c)
stays the same
20.

If pressure is held constant and "n" increases what happens to T?

a)

Increases

b)

Decreases

c)

Unchanged

21.

"n" and T have a(an) _________ relationship.

a)

Inverse

b)

Direct

22.

P and V have a(an) ________ relationship.

a)

Inverse

b)

Direct

23.

"n" and V have a(an) ________ relationship.

a)

Inverse

b)

Direct

24.

A direct relationship means as one increases the other _________.

a)

Increases

b)

Decreases

25.

An inverse relationship states that as one variable decreases the other __________.

a)

Increases

b)

Decreases

26.

Adding heat to a solid makes the particles move...

a)

Particles in a solid are not moving

b)

Slower

c)

At the same rate as before the heat was applied

d)

Faster

27.

The particles in a gas are ______ away from each other than the particles in a solid

a)

farther

b)

closer

c)

the same distance

28.

This one is tricky!

The temperature of each flask is given in Kelvin (K). Think about how temperature affects the motion of gas particles. Now think about what causes gas pressure....

Which of the following statements is correct?

a)

Flask 1 has the lowest pressure

b)

Flask 3 has the lowest pressure

c)

Flask 2 has the lowest pressure

d)

Flask 4 has the lowest pressure

29.

Which among the following is NOT true regarding the Kinetic Molecular Theory of gases?

a)

Gases particles move in straight lines.

b)

Gas particles are closely packed and their motion is orderly.

c)

Gas particles are in constant motion.

d)

Gas particles do not attract or repel each other.

30.

Which type of motion in the figure best represents the movement of gas particles?

a)

Motion 1

b)

Motion 2

c)

Motion 3

d)

Motion 4

31.
Of these three states of matter, which one has the most kinetic energy? 
a)
Solid 
b)
Liquid 
c)
Gas
32.

Which of the following statements is true?

a)

Gases do not move in straight line

b)

Gas particles are spaced so far apart that most of the volume of gas is empty space

c)

Gas particles are not in constant motion

d)

Gas particles attract each other

33.

The pressure of each flask is given in atmospheres (atm). Flask 1 has the lowest pressure, and Flask 4 has the highest. Knowing what causes gas pressure, which of the following statements is true?

a)

Flask 1 contain the most molecules

b)

Flask 2 contain the most molecules

c)

Flask 3 contain the most molecules

d)

Flask 4 contain the most molecules

34.

The energy of motion is known as ___.

a)

potential energy

b)

kinetic energy

c)

mechanical energy

35.
The movement of gas molecules is greatly affected by _________.
a)
the shape of the container
b)
size of the container
c)
temperature of the container
36.

Gas pressure is caused by ______.

a)

gravity.

b)

gas molecules colliding with each other.

c)

gas molecules colliding with surfaces of the container.

d)

gas molecules reacting with each other.

37.

What happens to matter as its temperature increases?

a)

The average kinetic energy of its particles decreases

b)

The average thermal energy of its particles decreases

c)

The particles gain kinetic energy

d)

The particles lose potential energy

38.
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.
39.
Does HCl have hydrogen bonding?
a)
yes
b)
no
40.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
41.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

42.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

43.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
44.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

45.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

46.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)
bond type
b)
density
c)
solubility
d)
molecular polarity
47.

Intermolecular Forces are the forces that exist

a)

Between two or more molecules

b)

Within a single molecule

c)

Only in molecules containing carbon

d)

In all molecules

48.

Examples of an intermolecular force include

a)

london disperson

b)

hydrogen bonding

c)

dipole dipole

d)

all of the above

49.

For hydrogen bonding to occur, a molecule must have a hydrogen bonded to

a)

carbon

b)

another hydrogen

c)

Fluorine, Chlorine or Oxygen

d)

Fluorine, Nitrogen or Oxygen

50.

Type of intermolecular force present in I2, Br2, and Cl2.

a)

dipole dipole

b)

H-bond

c)

London dispersion

d)

metallic

51.

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

52.

In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces

a)

Higher

b)

Lower

c)

The same

53.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

54.

The intermolecular force present in all matter is

a)

Hydrogen Bonding

b)

Ionic Bonding

c)

Dipole-Dipole

d)

London or Dispersion

55.

The strongest IMF is

a)

London/Dispersion

b)

Dipole-Dipole

c)

Hydrogen Bonding

56.

The weakest IMF is

a)

Dipole-Dipole

b)

Dispersion

c)

Hydrogen Bonding

57.

To form a hydrogen bonding, Hydrogen needs to attract to the highly electronegative elements such us _____, _____, and ____

a)

chlorine, fluorine, and oxygen

b)

fluorine, oxygen, and sulfur

c)

fluorine, bromine, and oxygen

d)

fluorine, oxygen, and nitrogen

58.

Dipole-Dipole forces are stronger than _______ and weaker than _________ interactions.

a)

london dispersion, ion-dipole

b)

hydrogen bonding, london dispersion

c)

ion-dipole, london dispersion

59.

Hydrogen bonding is a special case of __________.

a)

london dispersion

b)

ion-dipole

c)

dipole-dipole

60.

Which of the following has the lowest boiling point?

a)

PH3

b)

H2O

c)

SiH4

d)

NH3

61.

 Which of these has ONLY London forces?

a)

I2 (nonpolar)

b)

NH3 (polar)

c)

OCl2 (polar)

d)

HCl (polar)

62.

What intermolecular forces will be found between two of the molecules shown?

a)

dispersion forces only

b)

dispersion forces, dipole-dipole forces and hydrogen bonding

c)

dispersion forces and dipole-dipole forces

d)

dispersion forces and hydrogen bonding

63.

What intermolecular forces will be found between two of the molecules shown?

a)

dispersion forces only

b)

dispersion forces and dipole-dipole forces

c)

dispersion forces, dipole-dipole forces, and hydrogen bonding

d)

hydrogen bonding only

64.

What types of intermolecular forces will be present between two molecules of acetone?

a)

Dispersion forces only

b)

dipole-dipole forces & dispersion forces

c)

dispersion forces, dipole-dipole forces, and hydrogen bonding

d)

dispersion forces and hydrogen bonding

65.

Intermolecular force resulting from the attraction of partial positive and negative charges on polar molecules.

a)

dispersion force

b)

dipole-dipole force

c)

hydrogen bonding

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