At constant pressure,the temperature of $20 \ L$ of helium gas is increased from $100 \ K$ to $300 \ K$. What will be the change in volume in $L$?

An ideal gas expands isothermally and reversibly from $10 \ m^{3}$ to $20 \ m^{3}$ at $300 \ K$ performing $5.187 \ kJ$ of work on surroundings. Calculate the number of moles of gas undergoing expansion? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

Two closed vessels of equal volume containing air at pressure $P_1$ and temperature $T_1$ are connected to each other through a narrow tube. If the temperature in one of the vessels is now maintained at $T_1$ and that in the other at $T_2$,what will be the final pressure in the vessels?

At temperature $t \, ^oC$,the pressure exerted by $12 \, g$ of an ideal gas in a container of volume $V \, L$ is $1 \, atm$. When the temperature is increased by $10 \, ^oC$ without changing the volume,the pressure increases by $10 \%$. Find the temperature $t$ and volume $V$ in $L$. (Molar mass of the gas = $120 \, g/mol$)

In a $1 \ L$ flask,$N_2$ gas is at $100 \ kPa$ pressure,and in another $3 \ L$ flask,$O_2$ gas is at $320 \ kPa$ pressure. If both flasks are connected,what will be the resultant pressure in $kPa$?

$A$ gas occupies $11.2 \ dm^3$ at $105 \ kPa$. What is the volume if pressure is increased to $210 \ kPa$ (in $dm^3$)?