How do changes in temperature at constant pressure affect the distance between gas particles? a. the motion of gas particles decreases as temperature increases. b. a decrease in temperature increases the distance between gas particles. c. an increase in temperature increases the distance between gas particles. d. the distance between gas particles is only affected by changes in pressure.

Answer: option c. an increase in temperature increase the distance between gas particles.

Justification:

Remember that the kinetic energy of the particles is directly related with the temperature. So, as implication as the temperarue increase the kinetic energy increase.

After that remember that the kinetic energy is proportional to the square of the speed of the particles. So, an increase of kinetic energy is related with the increase of the speed of the particles.

Finally, reason that as the speed of the particles is higher the more apart they are and the gas will occupy more space (volume).

In the kinetic theory for ideal gases you do not take in account the intermolecular forces (they are supposed to be inexistent) but you do deal with the fact that the temperature increase the velocity of the molecules which means more speed and more free space among them.

I believe the answer is C. An increase in temperature increases the distance between gas particles. At constant pressure, when there is an increase in temperature the motion of the gas particles will increase. The effect is that increase in temperature increases the kinetic energy of gas molecules, making them move more faster and vibrate more. This will result to an increase in inter-molecular collision hence the molecules will move further and further away from each other.