$A$ gas is contained in a closed vessel. The initial temperature of the gas is $100^{\circ} C$. If the pressure of the gas is increased by $4 \%$,what is the increase in the temperature of the gas (in $^{\circ} C$)?

The equation of state for $2 \ g$ of oxygen at a pressure $P$ and temperature $T$,when occupying a volume $V$,will be:

Two vessels separately contain two ideal gases $A$ and $B$ at the same temperature. The pressure of $A$ is twice that of $B.$ Under such conditions,the density of $A$ is found to be $1.5$ times the density of $B.$ The ratio of the molecular weight of $A$ to that of $B$ is

One mole of an ideal gas undergoes a process $P = \frac{2V^2}{1+V^2} \, Pa$. The change in temperature of the gas when the volume changes from $V = 1 \, m^3$ to $V = 2 \, m^3$ is:

At a pressure $P$ and temperature $T$, $7 \text{ g}$ of oxygen occupies a volume $V$. The equation of state will be (Molecular weight of Oxygen = $32$).

An open container contains $x$ moles of gas at $T$ $K$. If the temperature is tripled,then the amount of gas that exits the container is: