At $127 \, ^oC$ temperature,the volume of a gas is $3 \, L$. If the volume of the gas becomes half at constant pressure,calculate the final temperature in Kelvin. (in $, K$)

At $300\, K$,the density of a certain gaseous molecule at $2\, bar$ is double that of dinitrogen $(N_2)$ at $4\, bar$. The molar mass of the gaseous molecule is ............... $g\, mol^{-1}$.

The density of a gas at $27\,^oC$ and $1\, atm$ is $d$. At constant pressure,which of the following temperatures will result in a gas density of $0.75\, d$?

For one mole of an ideal gas, the slope of $V$ vs. $T$ curve at a constant pressure of $2 \ atm$ is $X \ L \ mol^{-1} \ K^{-1}$. The value of the ideal universal gas constant '$R$' in terms of $X$ is

At a given temperature,the density of gas $x$ is twice the density of gas $y$. If the molar mass of $y$ is three times the molar mass of $x$,find the ratio of their pressures $(P_x/P_y)$.

Derive the relation between the density of gases and their molecular mass using Avogadro's law.