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 volume is made half of its original value keeping the temperature constant?

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Solution

Boyle’s Law describes the inverse proportional relationship between pressure and volume at a constant temperature and a fixed amount of gas. $P α \frac{1}{V}$
When, $V_{2} = \frac{1}{2} V_{1}$ ,
$P_{2} = \frac{2 P_{1} V_{1}}{V_{1}} \Rightarrow P_{2} = 2 P_{1}$
Pressure would be 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 volume is made half of its original value keeping the temperature constant?

Boyle’s Law describes the inverse proportional relationship between pressure and volume at a constant temperature and a fixed amount of gas. Pα1VWhen, V2=12V1, P2=2P1V1V1⇒P2=2P1Pressure would be doubled.

Boyle’s Law describes the inverse proportional relationship between pressure and volume at a constant temperature and a fixed amount of gas. $P α \frac{1}{V}$
When, $V_{2} = \frac{1}{2} V_{1}$ ,
$P_{2} = \frac{2 P_{1} V_{1}}{V_{1}} \Rightarrow P_{2} = 2 P_{1}$
Pressure would be doubled.