Volume occupied by a gas at $1 \, \text{atm}$ pressure and $0 \, ^\circ C$ is $V \, mL$. Its volume at $273 \, K$ will be

Four vessels of same volume consist of equal moles of four gases $H_2$,$Cl_2$,$N_2$,and $O_2$ separately at the same temperature. The pressure exerted by the gas is maximum for -

$A$ car tyre is filled with nitrogen gas at $35 \ \psi$ at $27^{\circ} C$. It will burst if pressure exceeds $40 \ \psi$. The temperature in $^{\circ} C$ at which the car tyre will burst is ............ (Rounded-off to the nearest integer)

$A$ gas at $10^{\circ}C$ occupies a volume of $283 \text{ mL}$. If it is heated to $20^{\circ}C$ at constant pressure, what is the new volume of the gas (in $\text{ mL}$)?

In $1811$,Avogadro calculated the formula of camphor by measuring the density of its vapour. Avogadro found the density to be $3.84 \ g/L$,when he made the measurement at $210 \ ^oC$ and $1 \ atm$ pressure. Which of the following is the correct formula of camphor?

At what temperature will the volume of a gas be halved if the initial temperature is $17^{\circ}C$ and the pressure remains constant (in $^{\circ}C$)?