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

Four vessels of same volume consist of equal moles of four gases $H_2$,$Cl_2$,$N_2$,and $O_2$ separately at the same temperature. The pressure exerted by the gas is maximum for -

Find the gas,if its density at $273 \ K$ temperature and $76 \ cm \ Hg$ pressure is $1.94 \ g / dm^3$.

The density of a gas is equal to ...... ($P =$ pressure,$V =$ volume,$T =$ temperature,$R =$ gas constant,$n =$ number of moles,and $M_w =$ molecular weight):

An open vessel at $27\,^{\circ}C$ is heated until two-fifths of the air (assumed as an ideal gas) in it has escaped from the vessel. Assuming that the volume of the vessel remains constant,the temperature to which the vessel has been heated is:

What is the temperature of $4$ moles of a gas occupying $5 \ L$ volume at $3.32 \ bar$ (in $K$)? $\left(R=0.083 \ bar \ L \ K^{-1} \ mol^{-1}\right)$