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12 Dec 2019

According to the kinetic molecular theory, if you increase the temperature of a gas without changing the volume of the gas, the particles of the gas will _______.

A strike the container walls more often

B strike the walls with less force

C lose kinetic energy

D increase in size

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Patrina Schowalter
Patrina SchowalterLv2
13 Dec 2019

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Related questions

1. The pressure of a gas result from?

a. gas particles colliding with each other.

b. gas particles colliding with the container walls.

c. the sum of the volumes of the particles being larger than the container volume.

Ā 

2. The temperature of a gas is a measure of what?

a. the kinetic energy of the gas particles.

b. the volumes of the gas particles.Ā 

c. the amount of space between gas particles.

d.Ā  the number of gas particles.

All of the following statements underlie the kinetic molecular theory of gases EXCEPT:

a. Gas molecules have no intermolecular forces.

b. Gas particles are in random motion.

c. Gas particles have no volume.

d. The average kinetic energy is proportional to the temperature ( ) of the gas.

Which statement is false?

A. The molecules of an ideal gas are relatively very far apart on the average.
B. At a given temperature, according to the kinetic molecular theory, the average velocity of He atoms is the same as the average velocity of F2 molecules.
C. The average kinetic energies of molecules of samples of different ideal gases at the same temperature are the same.
D. The molecules of a gas move in straight paths until they collide with other molecules or the walls of their containers, according to the kinetic molecular theory.

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