Answers26-27 CFISD TX-Chemistry A CRPeriodic Trends

Gases Answers

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The table describes a gas stored in four different containers. Properties of Stored GasContainerProperties1· Low number of collisions with container walls· Medium average kinetic energy· Large number of particles2· Large number of collisions with container walls· Medium average kinetic energy· Small number of particles with little spaces between them3· Large number of collisions with container walls· High average kinetic energy· Large number of particles with large spaces between them4· Few collisions with container walls· Low average kinetic energy· Small number of particlesWhich container has gas stored at the highest temperature?

A
1
B
2
C
3
D
4
2
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Which sequence represents the relationship between temperature and volume as explained by the kinetic-molecular theory?

A
higher temperature more kinetic energy more space between particles higher volume
Option A
B
higher temperature less kinetic energy less space between particles higher volume
Option B
C
higher temperature more kinetic energy less space between particles lower volume
Option C
D
higher temperature less kinetic energy more space between particles lower volume
Option D
3

A graph of gas pressure versus the number of particles in a container is a straight line. Which other relationship will have a similar graph?

A
volume versus pressure, because they are also directly proportional
B
volume versus temperature, because they are also directly proportional
C
volume versus pressure, because they are also inversely proportional
D
volume versus temperature, because they are also inversely proportional
4

Which observation indicates that the kinetic-molecular theory has limited use for describing a certain gas?

A
Gas particles are acting like tiny, solid spheres.
B
Gas particles are obeying Newton’s laws of motion.
C
Increasing pressure is reducing the volume of the gas.
D
Increasing collisions of gas molecules will increase energy between them.
5

Which step will decrease the pressure of a gas inside a closed cubical container?

A
increasing the number of moles of gas
B
decreasing the volume of the container
C
increasing the speed of the gas particles
D
decreasing the temperature inside the container
6

Which two conditions can limit the usefulness of the kinetic-molecular theory in describing gas behavior?

A
high pressure and low temperatures
B
high pressure and medium temperatures
C
low pressure and low temperatures
D
low pressure and medium temperatures
7

The closeness of particles of gas and their low speeds allow intermolecular forces to become important at certain pressures and temperatures. Which best describes this statement?

A
This is a limitation of the kinetic-molecular theory.
B
This is a postulate of the kinetic-molecular theory.
C
This describes ideal gas behavior using the kinetic-molecular theory.
D
This describes ideal gas behavior without the kinetic-molecular theory.
8

According to the kinetic-molecular theory, the collision between two ideal gas particles is a result of

A
neither attraction nor repulsion.
B
repulsion from the wall of the container.
C
repulsion from other gas particles.
D
attraction between the two particles.
9

Which statement describes effusion?

A
It occurs when a gas passes through a tiny hole.
B
It occurs when a liquid passes through a tiny hole.
C
It occurs when gas molecules disperse throughout a container.
D
It occurs when a liquid disperses throughout a container.
10

Which statement best describes the collisions of gas particles according to the kinetic-molecular theory?

A
When particles pass close enough to one another, their attractions pull them together, and then they bounce apart with no gain or loss of energy.
B
As particles travel in straight lines, their paths sometimes meet, and then they bounce apart with no gain or loss of energy.
C
When particles pass close enough to one another, their attractions pull them together, and then they bounce apart with a loss of energy.
D
As particles travel in straight lines, their paths sometimes meet, and then they bounce apart with a loss of energy.
11

Which step will decrease the pressure of a gas inside a closed cubical container?

A
increasing the number of moles of gas
B
decreasing the volume of the container
C
increasing the speed of the gas particles
D
decreasing the temperature inside the container
12

The closeness of particles of gas and their low speeds allow intermolecular forces to become important at certain pressures and temperatures. Which best describes this statement?

A
This is a limitation of the kinetic-molecular theory.
B
This is a postulate of the kinetic-molecular theory.
C
This describes ideal gas behavior using the kinetic-molecular theory.
D
This describes ideal gas behavior without the kinetic-molecular theory.
13

Which statement best describes the collisions of gas particles according to the kinetic-molecular theory?

A
When particles pass close enough to one another, their attractions pull them together, and then they bounce apart with no gain or loss of energy.
B
As particles travel in straight lines, their paths sometimes meet, and then they bounce apart with no gain or loss of energy.
C
When particles pass close enough to one another, their attractions pull them together, and then they bounce apart with a loss of energy.
D
As particles travel in straight lines, their paths sometimes meet, and then they bounce apart with a loss of energy.
14

Which observation indicates that the kinetic-molecular theory has limited use for describing a certain gas?

A
Gas particles are acting like tiny, solid spheres.
B
Gas particles are obeying Newton’s laws of motion.
C
Increasing pressure is reducing the volume of the gas.
D
Increasing collisions of gas molecules will increase energy between them.
15

Which statement about gases is true?

A
They are made up of particles that always move very slowly.
B
They are made up of particles that travel in a curved path when in motion.
C
They are made up of hard spheres that vibrate quickly in stationary positions.
D
They are made up of hard spheres that are in random motion.
16

Which statement best describes the compressibility of a gas?

A
Increasing the temperature of a gas decreases the pressure.
B
Increasing the temperature of a gas increases the pressure.
C
Increasing the pressure on a gas decreases the volume.
D
Increasing the pressure on a gas increases the volume.
17

The table describes a gas stored in four different containers. Properties of Stored GasContainerProperties1· Low number of collisions with container walls· Medium average kinetic energy· Large number of particles2· Large number of collisions with container walls· Medium average kinetic energy· Small number of particles with little spaces between them3· Large number of collisions with container walls· High average kinetic energy· Large number of particles with large spaces between them4· Few collisions with container walls· Low average kinetic energy· Small number of particlesWhich container has gas stored at the highest temperature?

A
1
B
2
C
3
D
4
18

According to the kinetic-molecular theory, the collision between two ideal gas particles is a result of

A
neither attraction nor repulsion.
B
repulsion from the wall of the container.
C
repulsion from other gas particles.
D
attraction between the two particles.
19

A graph of gas pressure versus the number of particles in a container is a straight line. Which other relationship will have a similar graph?

A
volume versus pressure, because they are also directly proportional
B
volume versus temperature, because they are also directly proportional
C
volume versus pressure, because they are also inversely proportional
D
volume versus temperature, because they are also inversely proportional
20

Which is an example of the kinetic-molecular theory not holding true for a gas?

A
The average kinetic energy of particles depends only on the temperature.
B
The particles in a gas travel in straight lines in a continuous, random motion.
C
The attraction between particles causes a gas to condense at low temperatures.
D
The particles in a gas make up a small portion of the total volume of the gas.

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