An ideal gas weighing $9.0 \ g$ occupies a volume of $8.2 \ L$ at $300 \ K$ and $1 \ atm$ pressure. The molar mass of the gas is .....

What is the molar volume of an ideal gas at $27\,^oC$ and $1\, atm$ pressure in $L$?

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 $300 \ K$,the following graph is obtained for one mole of an ideal gas. If its pressure is $10 \ atm$,then its volume (in $L$) will be

$A$ $3.7 \ g$ mass of a gas occupies a certain volume at $25 \ ^\circ C$. The same volume is occupied by $0.184 \ g$ of $H_2$ gas at the same pressure and $17 \ ^\circ C$. Calculate the molar mass of the gas.

If $2.5$ moles of an ideal gas at a certain temperature are allowed to expand isothermally and reversibly from an initial volume of $2$ $dm^3$ to $20$ $dm^3$,the work done by the gas is $-16.5$ $kJ$. The temperature (in $K$) of the gas is (Round off to the nearest value). $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$