In the equation $PV = nRT$,the number of moles per liter can be expressed as:

At $300 \, K$ temperature and $1 \, atm$ pressure,the volume of $7.0 \, g$ of a gas is $4.1 \, L$. What is the molar mass of the gas?

The variation of volume of an ideal gas with its number of moles $(n)$ is obtained as a graph at $300 \ K$ and $1 \ atm$ pressure. What is the slope of the graph?

What is the volume in $litre$ occupied by $7 \, g$ of $N_2$ gas at $27 \, ^oC$ temperature and $750 \, mm \, Hg$ pressure?

$A$ vessel contains $3.2 \ g$ of dioxygen gas at $STP$ ($273.15 \ K$ and $1 \ atm$ pressure). The gas is now transferred to another vessel at constant temperature,where pressure becomes one third of the original pressure. The volume of the new vessel in $L$ is $........$ (Given: molar volume at $STP$ is $22.4 \ L$)

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). $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$