The change in internal energy of a mass of gas, when the volume changes from $V$ to $2V$ at constant pressure $P$ is (where $\gamma$ is the ratio of specific heat at constant pressure to that at constant volume, $\gamma = \frac{C_p}{C_v}$):

Describe the nature of $P-V$ diagrams for isobaric and isochoric processes.

$A$ monoatomic gas $(\gamma = 5/3)$ expands at constant pressure when heat is supplied. What percentage of the heat supplied is converted into internal energy and work, respectively?

When the temperature of $1 \, \text{mole}$ of an ideal gas is increased from $0^{\circ}C$ to $100^{\circ}C$ at constant pressure, what is the work done during the process? $(R = 8.3 \, J/mol \cdot K)$

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 $J$)

In Column-$I$ a graph and in Column-$II$ processes are given. Match them appropriately:

Column-$I$	Column-$II$
$(a)$ Graph $(a)$	$(i)$ Adiabatic process
$(b)$ Graph $(b)$	$(ii)$ Isobaric process
	$(iii)$ Isochoric process