If the absolute temperature of a gas is doubled and the pressure of the gas is halved how will the volume change? Will it increase by 4 times its original value or will it decrease to one forth of its original value

Are you familiar with the Ideal Gas law?


PV = nRT

Rearrange it: \frac {PV}{T} = nR

Given the number of moles of gas is constant, then \frac {PV} T is a constant. Hence:

\frac {P_1 V_1}{T_1} = \frac {P_2 V_2}{T_2}

So if P_2 = \frac 1 2 P_1, and T_2 = 2 \times T_1, what value must V_2 be?

Thanks a lot, I was solving it the wrong way. Now, I got it right.