The rate of diffusion of methane $(CH_4)$ at a given temperature is twice that of gas $X$. The molecular weight of gas $X$ is:

At a certain temperature, the time required for the complete diffusion of $200 \ mL$ of $H_2$ gas is $30 \ min$. The time required for the complete diffusion of $50 \ mL$ of $O_2$ gas at the same temperature will be: (in $min$)

The ratio of densities of two gases is $1:16$. What will be the ratio of their rates of diffusion?

What will be the pressure at $0\,^oC$ in Kolkata,Chennai,and Mumbai (in $,bar$)?

Calculate the ratio of the effusion of $CO$ and $N_2$,when temperature and pressure gradients are held constant?

$3.2 \, g$ of oxygen gas diffuses in $10 \, minute$. Under similar conditions,$2.8 \, g$ of nitrogen gas will diffuse in ............ $minute$.