Question

Flask $A$ contains $H_2$ gas and $B$ contains $C{H}_4$ gas have equal mass and volume at 300 $K$ and 600 $K$ respectively. Which flask has the highest pressure?

Assuming ideal behaviour for both the gases.

• A. $A$
• B. $B$
• C. Both $A$ and $B$ are equal
• D. Data insufficient

Answer 1

The correct option is A $A$

From Ideal gas equation,

$PV=nRT$

Given,

$T_A=300K$
$T_B=600K$

Since,

$P_{A}V=n_{A}R{T}_A$

$P_{B}V=n_{B}R{T}_B$

$\therefore \frac{P_A}{P_B}=\frac{n_A{T}_A}{n_B{T}_B}$

$\frac{P_A}{P_B}=\frac{m\times 16\times T_A}{m\times 2\times T_B}$

$\frac{P_A}{P_B}=8\times \frac{300}{600}=4$

$\therefore P_A>P_B$ or $P_A=4P_B$

Hence, option $\left(A\right)$ is correct.