A thermodynamic system is taken from an original state to an intermediate state by the linear process shown in Figure.

Its volume is then reduced to the original value from $E$ to $F$ by an isobaric process. Calculate the total work done (in $J$) by the gas from $D$ to $E$ to $F$

In the diagrams $(i)$ to $(iv)$ of variation of volume with changing pressure is shown. A gas is taken along the path $ABCD. $ The change in internal energy of the gas will be

Find the amount of work done to increase the temperature of one mole of an ideal gas by $30^o\ C$ if it is expanding under the condition  …. $J$

$V\propto {T^{\frac{2}{3}}}$ $[R = 1.99\  cal/mol-K]$

An ideal gas goes from state $A$ to state $B$ via three different processes as indicated in the $P-V$ diagram. If $Q_1, Q_2, Q_3$ indicate the heat absorbed by the gas along the three processes and $\Delta U_1, \Delta U_2, \Delta U_3$ 
indicate the change in internal energy along the three processes respectively, then 

An enclosed ideal gas is taken through a cycle as shown in the figure. Then