An air bag on adiabatic expansion undergoes $5 \%$ increase in its volume. The percentage change in pressure is $\left[\gamma_{air}=1.4\right]$ (in $\%$)

At $27\,^{\circ}C$ temperature and $4\, bar$ pressure,$CO_2$ is filled in a $2\, L$ vessel. Find the pressure if it is filled in a $4\, L$ vessel at $77\,^{\circ}C$ temperature. (in $, bar$)

The temperature of $1 \, mol$ of a gas is increased by $2 \, ^oC$ at constant pressure. The work done will be:

Two separate bulbs contain ideal gases $A$ and $B$. The density of gas $A$ is twice that of gas $B$. The molecular mass of $A$ is half that of gas $B$. The two gases are at the same temperature. The ratio of the pressure of $A$ to that of gas $B$ is

If two moles of an ideal gas at $546 \ K$ occupy a volume of $44.8 \ L$,what is the pressure of the ideal gas at $546 \ K$ (in $atm$)? $(R = 0.0821 \ L \ atm \ mol^{-1} \ K^{-1})$

In the equation $PV = nRT$,which one cannot be the numerical value of $R$?