If the density of a gas at $NTP$ is $0.00445 \ g/mL$,then its vapor density and molecular weight are respectively:

Which of the following equations is correct for the vapour density of completely dissociated ammonium chloride?

For the reaction $A_{3(g)} \rightleftharpoons 3A_{(g)}$,the initial moles of $A_3$ is $a$. If $\alpha$ is the degree of dissociation of $A_3$,then the total number of moles at equilibrium will be:

Consider the reaction $X_2Y_{(g)} \rightleftharpoons X_{2(g)} + \frac{1}{2}Y_{2(g)}$. The equation representing the correct relationship between the degree of dissociation $(x)$ of $X_2Y_{(g)}$ with its equilibrium constant $Kp$ is. . . . . . . Assume $x$ to be very very small.

At $T \, ^\circ C$,the vapour density of $PCl_5$ is $104.25$. The degree of dissociation of $PCl_5$ is ....$\%$

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$; if $K_C = 2$,then the degree of dissociation of $O_2$ is: