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:

$A$ large flask contains air at $27 \, ^{\circ}C$. In order to expel half the mass of air from the flask, the flask should be heated up to what temperature in $^{\circ}C$?

$A$ gas at absolute temperature $300\,K$ has pressure $P = 4 \times 10^{-10}\,N/m^2$. Given the Boltzmann constant $k = 1.38 \times 10^{-23}\,J/K$,the number of molecules per $cm^3$ is of the order of:

For a given mass of a gas at constant temperature, the volume and the pressure are $V$ and $P$ respectively. Then the slope of the graph drawn between $\log_e V$ on the $X$-axis and $\log_e P$ on the $Y$-axis is

The figure shows the $P-V$ diagram of two different masses $m_1$ and $m_2$ of the same gas drawn at a constant temperature $T$. Then:

In the relation $n = \frac{PV}{RT}$,what does $n$ represent?