The vapour density of a mixture containing $NO_2$ and $N_2O_4$ is $27.6$. The mole fraction of $N_2O_4$ in the mixture is

At $NTP$,$5.6 \ L$ of a gas weighs $8 \ g$. The vapour density of the gas is:

The equilibrium constant at a certain temperature for the reaction $A_2 + B_2 \rightleftharpoons 2AB$ is $2$. Calculate the degree of dissociation of either $A_2$ or $B_2$.

The value of $K_P$ for the equilibrium reaction ${N_2}{O_4}_{(g)} \rightleftharpoons 2N{O_2}_{(g)}$ is $2$. The percentage dissociation of ${N_2}{O_4}_{(g)}$ at a pressure of $0.5 \ atm$ is

For the reaction $A \rightleftharpoons \frac{1}{2} B + C$,the degree of dissociation $\alpha$ in terms of vapour density $D_t$ (theoretical) and $D_o$ (observed) is given by:

$A$ gas has the formula $[CO]_x$. If its vapor density is $70$,what is the value of $x$?