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WorksheetsKMT and IMF (no phase diagrams or heating curves)
Total questions: 43
Worksheet time: 59mins
Name
Class
Date
1.
An exothermic reaction:
a)
Produces heat when the reaction occurs
b)
Absorbs heat when a reaction occurs
2.
An endothermic reaction
a)
Produces heat when a reaction occurs
b)
Absorbs heat when a reaction occurs
3.
Which sample has hydrogen bonding?
a)
H2S
b)
CH4
c)
NH3
d)
HI
4.
Water has an unusually high boiling point for a molecular compound because it has
a)
hydrogen bonding
b)
ion-ion attractions
c)
a high density
d)
a large gram formula mass
5.
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
6.
The weaker the intermolecular forces of a substance the _____________ the boiling point
a)
higher
b)
lower
7.
________________________ have the strongest intermolecular forces of attraction.
a)
Dipole- Dipole
b)
Dispersion
c)
Hydrogen Bonds
8.
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
9.
Which of these has dispersion forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
10.
Intermolecular forces for: NH3
a)
Dispersion Force
b)
Dipole dipole
c)
Hydrogen bonding
11.
Thermal energy ALWAYS moves from _____ to _____.
a)
solid to liquid
b)
ice to water
c)
hot to cold
d)
solid to gas
12.
Which of the following terms identifies the change from a liquid to gas?
a)
Evaporation
b)
Condensation
c)
Melting
d)
Freezing
13.
Which of the following terms identifies the change from a liquid to solid?
a)
Melting
b)
Condensation
c)
Evaporation
d)
Freezing
14.
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
15.
Phase change from a solid to a liquid.
a)
melting
b)
freezing
c)
evaporation
d)
condensation
16.
When the temperature of matter decreases the particles ...
a)
speed up and move farther apart
b)
speed up and move closer together
c)
slow down and move farther apart
d)
slow down and move closer together
17.
Phase change from a gas to a liquid.
a)
condensation
b)
evaporation
c)
melting
d)
freezing
18.
The opposite phase of melting is
a)
freezing
b)
evaporation
c)
condensation
d)
deposition
19.
The phase change from water vapor to liquid water is known as...
a)
evaporation
b)
precipitation
c)
condensation
d)
sublimation
20.
What is it called when a solid turns directly into a gas?
a)
Sublimation
b)
Condensation
c)
Liquid
21.
Change from liquid to solid is call......
a)
fusion
b)
Freezing
c)
sublimation
d)
evaporation
22.
Change from liquid to gas is called....
a)
expansion
b)
evaporation
c)
condensation
d)
sublimation
23.
All changes in the state of matter of a substance requires...
a)
vibration
b)
water
c)
permission
d)
energy
24.
When a puddle of water dries up this process is called...
a)
Condensation
b)
Evaporation
c)
Melting
d)
Boiling
25.
Which two phases changes takes away energy?
a)
Freezing, Melting
b)
Condensation, Evaporation
c)
Freezing, Condensation
d)
Melting, Evaporation
26.
Which two phases changes add energy?
a)
Freezing, Melting
b)
Condensation, Evaporation
c)
Freezing, Condensation
d)
Melting, Evaporation
27.
What happens to particle movement/speed when energy is added to a phase?
a)
Particles slow down
b)
Particles go faster
c)
Particles don't move
d)
Particles stay the same speed
28.
Gas pressure is caused by
a)
gas molecules colliding with surfaces
b)
gas molecules condensing to a liquid
c)
gas molecules hitting other gas molecule
d)
barometers
29.
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
30.
a)
Flask 1 contain the least pressure
b)
Flask 2 contain the least pressure
c)
Flask 3 contain the least pressure
d)
Flask 4 contain the least pressure
31.
a)
Since all flask have same amount of gas, flask 1 has the least pressure
b)
Since all flask have same amount of gas, flask 2 has the least pressure
c)
Since all flask have same amount of gas, flask 3 has the least pressure
d)
Since all flask have same amount of gas, flask 4 has the least pressure
32.
a)
Gas particles are elastic and do not attract each other.
b)
The kinetic energy of gas is dependent on temperature
c)
Energy is not lost when gas particles collide with each other or with the walls of the container.
d)
All of the above
33.
Which among the following is not a property of gases?
a)
high compressible
b)
thermally expandable
c)
infinitely miscible
d)
high density
34.
Kinetic Energy means...
a)
energy that a body possesses by virtue of being in motion.
b)
energy that a body possesses by stored energy due to height.
c)
energy stored in the bonds ofchemical compounds.
d)
radiant energy emitted by the sun
35.
Movement of gas through a tiny opening
a)
Diffusion
b)
Effusion
36.
What is the lightest gas in the Periodic Table of Elements?
a)
Helium
b)
Oxygen
c)
Hydrogen
d)
Neon
37.
One assumption in KMT is that particles move in random straight line motion.
a)
True
b)
False
38.
Which of the following changes to a system WILL NOT result in an increase in pressure?
a)
Increasing the volume of the container
b)
Decreasing the volume of the container
c)
Adding more gas molecules
d)
Raising the temperature
39.
Dalton's Law states...
a)
that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.
b)
that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases
c)
how gases tend to expand when heated
d)
that the density of an ideal gas at constant pressure varies inversely with the absolute temperature of the gas.
40.
Which of the following gases will effuse most slowly under the same physical conditions?
Don't forget to check for diatomics!
Don't forget to check for diatomics!
a)
Hydrogen
b)
Chlorine
c)
Ammonia (NH3)
d)
Bromine
41.
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
42.
In order to calculate the rate of effusion of a gas, you must compare it to that of another gas and
a)
take the square root of the molar mass of the lighter gas divided by the square root of the molar mass of the heavier gas.
b)
take the square root of the molar mass of the heavier gas.
c)
take the square root of the molar mass of the lighter gas.
d)
take the square root of the molar mass of the heavier gas divided by the square root of the molar mass of the lighter gas.
43.
Heavier gases have a __________________ rate of effusion.
a)
Faster
b)
Slower
c)
Rate of effusion does not depend on mass.
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