$A$ gaseous mixture was prepared by taking equal moles of $CO$ and $N_2$. If the total pressure of the mixture was found to be $1 \ atm$,the partial pressure of the nitrogen $(N_2)$ in the mixture is ............ $atm$.

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 $x$)

The ratio of rates of diffusion of gases $X$ and $Y$ is $1:5$ and that of $Y$ and $Z$ is $1:6$. The ratio of rates of diffusion of $Z$ and $X$ is

$x \ g$ of molecular oxygen $(O_2)$ is mixed with $200 \ g$ of neon $(Ne)$. The total pressure of the nonreactive mixture of $O_2$ and $Ne$ in the cylinder is $25 \ bar$. The partial pressure of $Ne$ is $20 \ bar$ at the same temperature and volume. The value of $x$ is $....$ [Given: Molar mass of $O_2 = 32 \ g \ mol^{-1}$. Molar mass of $Ne = 20 \ g \ mol^{-1}$]

According to Graham's law at a given temperature,the ratio of the rates of diffusion ${r_A}/{r_B}$ of gases $A$ and $B$ is given by

On a certain day,the humidity in the atmosphere is $1\%$. If the barometer reads $760 \ mm \ of \ Hg$,what will be the pressure of the dry gas in $mm \ of \ Hg$?