Question

If one mole of $H_2$ gas is occupies a rigid container with a capacity of $1000$ litres and the temperature is raised from ${27}^{o}C$ to ${37}^{o}C$, the change in pressure of the contained gas (round off to two decimal places), assuming ideal gas behaviour, is $Pa$$(R=8.314J/mol-K)$

• A. 83.14

Answer 1

The correct option is A 83.14
$V=\text{Volume of rigid container}$

$T_1=\text{Initial temperature of the gas}$

$T_2=\text{Final temperature of the gas}$

$P_{1}V=n\overline{R}{T}_1$

$P_{2}V=n\overline{R}{T}_2$

$(P_2-P_1)V=n\overline{R}(T_2-T_1)$

$\Delta P\times 1=1\times 8.314(37-27)$

$\Delta P=83.14Pa$