$A$ monoatomic gas is supplied heat $Q$ very slowly while keeping the pressure constant. The work done by the gas will be

If $R$ is the universal gas constant,the amount of heat needed to raise the temperature of $2$ moles of an ideal monoatomic gas from $273 \ K$ to $373 \ K$ when no work is done is: (in $R$)

How much work is to be done in decreasing the volume of an ideal gas by an amount of $2.4 \times 10^{-4} \ m^3$ at normal temperature and constant normal pressure of $1 \times 10^5 \ N/m^2$ (in $J$)?

Match the graphs in Column-$I$ with the processes in Column-$II$:

Column-$I$	Column-$II$
$(a)$ Horizontal line parallel to $V$-axis	$(i)$ Adiabatic process
$(b)$ Vertical line parallel to $P$-axis	$(ii)$ Isobaric process
	$(iii)$ Isochoric process

Two moles of helium gas are taken over the cycle $ABCDA$,as shown in the $P-T$ diagram. Assuming the gas to be ideal,the work done on the gas in taking it from $A$ to $B$ is ...... $R$.

When an ideal gas $(\gamma = 5/3)$ is heated under constant pressure,what percentage of the given heat energy will be utilized in doing external work (in $\%$)?