$A$ given mass of a gas expands from a state $A$ to the state $B$ by three paths $1, 2$ and $3$ as shown in the $T-V$ indicator diagram. If $W_1, W_2$ and $W_3$ respectively be the work done by the gas along the three paths,then

The figure given below shows the variation in the internal energy $U$ with volume $V$ of $2.0 \text{ mole}$ of an ideal gas in a cyclic process $abcda$. The temperatures of the gas during the processes $ab$ and $cd$ are $500 \text{ K}$ and $300 \text{ K}$ respectively. The heat absorbed by the gas during the complete process is .... $J$. (Take $R = 8.3 \text{ J/mol-K}$ and $\ln 2 = 0.69$)

What is the nature of the change in internal energy for the following three thermodynamic processes shown in the figure?

$A$ system goes from $A$ to $B$ via two processes $I$ and $II$ as shown in the figure. If $\Delta U_I$ and $\Delta U_{II}$ are the changes in internal energies in the processes $I$ and $II$ respectively,then:

$A$ cyclic process for $1 \, \text{mole}$ of an ideal gas is shown in the figure in the $V-T$ diagram. The work done in $AB$, $BC$, and $CA$ respectively is:

Calculate the heat absorbed by the system in going through the process shown in the figure.