The molecular theory states that the pressure exerted by a gas in a closed vessel results from the gas molecules striking against the walls of the vessel. How will the pressure change if the temperature is doubled keeping the volume constant?

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Solution

When volume is kept constant, $P \propto T$ , i.e., pressure is directly proportional to temperature, hence, on doubling temperature pressure will also get doubled.

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The molecular theory states that the pressure exerted by a gas in a closed vessel results from the gas molecules striking against the walls of the vessel. How will the pressure change if the temperature is doubled keeping the volume constant?

When volume is kept constant, P∝T, i.e., pressure is directly proportional to temperature, hence, on doubling temperature pressure will also get doubled.

When volume is kept constant, $P \propto T$ , i.e., pressure is directly proportional to temperature, hence, on doubling temperature pressure will also get doubled.