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 the surroundings. Calculate the number of moles of gas used.

$A$ gas cylinder can withstand a pressure of $15 \ atm$. At $27 \ ^oC$,the pressure in the cylinder is $12 \ atm$. Up to what temperature in $^oC$ will the cylinder not burst?

An evacuated glass vessel weighs $40.0 \ g$ when empty,$135.0 \ g$ when filled with a liquid of density $0.95 \ g \ mL^{-1}$ and $40.5 \ g$ when filled with an ideal gas at $0.82 \ atm$ at $250 \ K$. The molar mass of the gas in $g \ mol^{-1}$ is .... .
(Given : $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$ )

Calculate the weight of $CH_4$ in a $9 \ L$ cylinder at $16 \ atm$ and $27 \ ^\circ C$ in grams.

$A$ dry gas occupied $127.4 \, mL$ at $STP$. If the same mass of the gas is collected over water at $27 \, ^\circ C$ and at a total pressure of $725 \, torr$,what volume does it occupy? The vapour pressure of water at $27 \, ^\circ C$ is $25 \, torr$. (Note: $1 \, bar = 750 \, torr$)

Find the temperature in $^\circ C$ for a $6.4 \ g$ $O_2$ gas filled in a $200 \ mL$ vessel having pressure $50 \ bar$. $[R = 8.314 \times 10^{-2} \ bar \ L \ K^{-1} \ mol^{-1}]$ (in $^\circ C$)