The value of $PV/T$ for one mole of an ideal gas is nearly equal to . . . . . . $J$ $mol^{-1}K^{-1}$.

When the temperature of a gas in a closed vessel is increased by $1^{\circ}C$,its pressure increases by $0.4\%$. The initial temperature of the gas is ...

Absolute zero $(0\, K)$ is that temperature at which

The figure shows the pressure $P$ versus volume $V$ graphs for two different gas samples at a given temperature. $M_A$ and $M_B$ are the masses of the two samples,and $n_A$ and $n_B$ are the numbers of moles. Which of the following must be incorrect?

When the temperature of a gas in a closed vessel is increased by $2.4^{\circ} C$, its pressure increases by $0.5 \%$. The initial temperature of the gas is (in $^{\circ} C$)

Column-$I$ represents a graph and Column-$II$ represents a physical quantity or condition that is constant for that graph. Match them correctly:

Column-$I$	Column-$II$
$(a)$ Top graph	$(i)$ Constant pressure
$(b)$ Bottom graph	$(ii)$ Constant volume
	$(iii)$ For ideal gas