In thermodynamics,for an isochoric process,which one of the following statements is $INCORRECT$?

The percentage of heat supplied to a diatomic ideal gas that is converted into work in an isobaric process is

Two containers $A$ and $B$ with pistons contain a diatomic gas at $300\, K$. The piston in container $A$ is free to move,while the piston in container $B$ is fixed. Both containers are supplied with the same amount of heat. If the temperature in container $A$ increases by $30\, K$,by how many $K$ will the temperature in container $B$ increase? Both containers contain the same gas.

The temperature of $1$ mole of an ideal monoatomic gas is increased by $50^{\circ} C$ at constant pressure. The total heat added and change in internal energy are $E_1$ and $E_2$,respectively. If $\frac{E_1}{E_2}=\frac{x}{9}$,then the value of $x$ is . . . . . . .

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 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 $J$)