$A$ sample of gas expands from volume ${V_1}$ to ${V_2}$. The amount of work done by the gas is greatest when the expansion is

The volume $(V)$ of a monatomic gas varies with its temperature $(T)$,as shown in the graph. The ratio of work done by the gas to the heat absorbed by it,when it undergoes a change from state $A$ to state $B$,is

Two moles of ideal helium gas are in a rubber balloon at $30^{\circ} C$. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to $35^{\circ} C$. The amount of heat required in raising the temperature is nearly (take $R = 8.31 \ J / mol \cdot K$) (in $J$)

$A$ diatomic gas $\left(C_P = \frac{7}{2} R\right)$ does $200 \ J$ of work when it is expanded isobarically. The heat given to the gas in the process is (in $J$)

Obtain the expression for work done by a gas during an isobaric process (constant pressure).

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 ...... $R$.