A gas has experienced a small increase in volume but has maintained the same pressure and number of moles. According to the ideal gas law, how has the temperature of the gas changed?

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Chemistry

5 April, 21:59

A gas has experienced a small increase in volume but has maintained the same pressure and number of moles. According to the ideal gas law, how has the temperature of the gas changed?

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Yusuf Spencer · Answer 1

Temperature has increased

Ideal Gas Law:

pressure * volume = (number of moles of gas) * (0.08206) * (temperature)

or short-hand:

PV = nRT

this equation can be transformed to solve for temperature as:

T = PV / nR

given there is no change in pressure and the volume of the container has increased, we know the temperature increases because volume is in the numerator--a larger number on top reflects an overall greater number.