Describe the relationship between volume and temperature of an ideal gas, and explain it in terms of the kinetic molecular theory of gases.

As temperature increases, the particles will gain kinetic energy causing it to move more rapidly and randomly. However, this causes the gas to expand as the particles will have more energy to roam freely. Hence as temperature increases, Volume increases.

This is based on Charles' Law stating that the volume of a gas is directly proportional to its absolute temperature.

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Annainn Annainn · Answer 2 · 2019-07-23T20:46:20+02:00

Answer:

Charles Law: V/T = constant

Explanation:

The ideal gas equation relates the pressure (P), temperature (T) and volume (V) of 'n' moles of a gas through the following equation:

[tex]PV = nRT[/tex]

where R = universal gas constant = 0.0821 Latm/mol-K

As per the kinetic molecular theory, an increase in temperature will increase the kinetic energy of the gas particles thereby increasing the rate of collision. Under constant pressure conditions, the volume would have to increase so as to reduce the rate of collisions. This implies that the volume (V) is directly proportional to the temperature (T).

[tex]V\alpha T[/tex]

i.e. [tex]V/T = constant[/tex]

This is referred to as Charles' Law