Question

Consider a balloon that has a volume V. It contains n moles of gas, it has an internal pressure of P, and its temperature is T. If the balloon is heated to a temperature of 15.5T while it is placed under a high pressure of 15.5P, how does the volume of the balloon change?

Answer 1

B.) it stays the same

Answer 2

Answer: The temperature will not change and will remain T.

Explanation: Accoding to ideal gas law:

$PV=nRT$

where,

P = pressure of the gas

V = volume of the gas

T = temperature of the gas

n = number of moles of gas

R = Gas constant = 0.0821 Latm/moleK

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

$P_1$= initial pressure

$V_1$= initial volume

$T_1$= initial temperature

$P_2$= final pressure

$V_2$= final volume

$T_2$= final temperature

Putting in the values:

$\frac{PV}{T}=\frac{15.5PV_2}{15.5T}$

$T_2=T$