If the temperature of a fixed mass of gas is increased by $1\,^{\circ}C$ at constant pressure,what will be the new volume of the gas?

$A$ $5.75 \ g$ sample of a gas occupies $3.5 \ L$ at $55 \ ^oC$ and $0.940 \ atm$ pressure. What is the molecular weight of the gas?

$A$ sample of gas occupies a volume of $0.2 \, L$ at $1 \, atm$ pressure and $0 \, ^oC$ temperature. What will be its volume in $L$ at the same pressure but at $273 \, ^oC$ temperature?

At $240.55 \ K$,for one mole of an ideal gas,a graph of $P$ (on $y$-axis) and $V^{-1}$ (on $x$-axis) gave a straight line passing through the origin. Its slope $(m)$ is $2000 \ J \ mol^{-1}$. What is the kinetic energy (in $J \ mol^{-1}$) of the ideal gas?

Pressure of $1 \, g$ of an ideal gas $A$ at $27^{\circ} C$ is found to be $2 \, bar$. When $2 \, g$ of another ideal gas $B$ is introduced in the same flask at the same temperature,the pressure becomes $3 \, bar$. Find a relationship between their molecular masses.

If the absolute temperature of an ideal gas becomes double and the pressure becomes half,the volume of the gas would be: