The volume of a gas at pressure $21 \times 10^4 \ N/m^2$ and temperature $27^\circ C$ is $83 \ L$. If $R = 8.3 \ J/mol/K$,then the quantity of gas in $gm-mole$ will be:

$A$ gas is heated through $1\,^{\circ}C$ in a closed vessel. Its pressure is increased by $0.5\%$. The initial temperature of the gas is ...... $^{\circ}C$.

$A$ gas at a temperature of $27^{\circ}C$ has a volume $V$ and pressure $P$. If the pressure is doubled and the volume is tripled,what will be the new temperature in $^{\circ}C$?

$A$ perfect gas at $27^\circ C$ is heated at constant pressure to $327^\circ C$. If the original volume of the gas at $27^\circ C$ is $V$,then the volume at $327^\circ C$ is:

$1$ mole of gas occupies a volume of $100\, ml$ at $50\, mm$ pressure. What is the volume occupied by two moles of gas at $100\, mm$ pressure and at the same temperature? (in $ml$)

An oxygen cylinder of volume $30 \; L$ has an initial gauge pressure of $15 \; atm$ and a temperature of $27 \; ^{\circ}C$. After some oxygen is withdrawn from the cylinder,the gauge pressure drops to $11 \; atm$ and its temperature drops to $17 \; ^{\circ}C$. Estimate the mass (in $kg$) of oxygen taken out of the cylinder ($R = 8.31 \; J \; mol^{-1} K^{-1}$,molecular mass of $O_{2} = 32 \; u$).