Question

A balloon contains $1500m^3$ of helium at $27{}^{\circ }C$ and 4 atmospheric pressure. The volume of helium at $-3{}^{\circ }C$ and 2 atmospheric pressure will be

• A. $1500m^3$
• B. $1700m^3$
• C. $1900m^3$
• D. $2700m^3$

Answer 1

Answer: (D)

$V_1=1500m^3,T_1=27{}^{\circ }C=300K$
$P_1=4atm,T_2=-3{}^{\circ }C=270K,P_2=2atm$
According to ideal gas equation, $\frac{P_1{V}_1}{T_1}=\frac{P_2{V}_2}{T_2}$
$\therefore V_2=\frac{P_1{V}_1}{T_1}\times \frac{T_2}{P_2}=\frac{4\times 1500\times 270}{300\times 2}=2700m^3$