$A$ gas at $27^{\circ}C$ has a volume $V$ and pressure $P$. If it is heated such that the pressure becomes double and the volume becomes triple,what is the final temperature in $^{\circ}C$?

What is the mass of $2$ litres of nitrogen gas $(N_2)$ at $22.4$ atmospheric pressure and $273\,K$?

$A$ tyre of a vehicle is filled with air having pressure $270 \text{ kPa}$ at $27^{\circ}C$. The air pressure in the tyre when the temperature increases to $37^{\circ}C$ is (in $\text{ kPa}$)

$A$ container $A$ contains an ideal gas at pressure $P$,volume $V$,and temperature $T$. $A$ second container $B$ contains the same gas at pressure $2P$,volume $2V$,and temperature $\frac{T}{2}$. The ratio of the mass of gas in $A$ to that in $B$ is:

The $SI$ unit of universal gas constant is

The adjoining figure shows the graph of pressure $(P)$ and volume $(V)$ of a gas at two temperatures $T_1$ and $T_2$. Which of the following inferences is correct?