The rate of diffusion of a gas $A$ is $\sqrt{5}$ times more than that of gas $B$. If the molar mass of $A$ is $x \ g \ mol^{-1}$,the molar mass of $B \ (\text{in } g \ mol^{-1})$ is (in $x$)

$A$ mixture of hydrogen and oxygen contains $40 \%$ hydrogen by mass when the total pressure is $2.2 \, bar$. The partial pressure of hydrogen is $bar$. (Nearest Integer)

At $T \ K$,equal weights of $H_2, D_2$,and $T_2$ are present in a closed vessel. The pressure exerted by this gaseous mixture is $P \ atm$. The ratio of partial pressures of $T_2, D_2$,and $H_2$ is approximately. ($H, D$ and $T$ are isotopes of hydrogen).

$A$ gaseous mixture of $2$ moles of $A$,$3$ moles of $B$,$5$ moles of $C$,and $10$ moles of $D$ is contained in a vessel. Assuming that gases are ideal and the partial pressure of $C$ is $1.5 \ atm$,what is the total pressure (in $atm$)?

Under similar conditions of temperature and pressure,$50 \ mL$ of gas $A$ diffuses through a hole in the same time that $40 \ mL$ of gas $B$ diffuses. If the molar mass of gas $A$ is $64$,what is the molar mass of gas $B$?

$A$ bulb contains $1 \ g$ of $H_2$ and $1 \ g$ of $He$. If the total pressure is $1.2 \times 10^3 \ Pa$,then the partial pressure of $He$ is ............. $Pa$.