Ammonium carbamate $(NH_2COONH_4)$ when heated to $200\,^{\circ}C$ gives a mixture of $NH_3$ and $CO_2$ with a vapour density of $13.0$ at equilibrium. What is the degree of dissociation of ammonium carbamate?

For the thermal dissociation of $PCl_5$ as $PCl_5 \rightleftharpoons PCl_3 + Cl_2$,if '$a$' moles of $PCl_5$ are taken and at equilibrium,the degree of dissociation of $PCl_5$ is $0.25$ and the total pressure is $2.0 \ atm$,then the partial pressure of $Cl_2$ at equilibrium will be: (in $atm$)

At temperature,$T$,a compound $AB_{2(g)}$ dissociates according to the reaction; $2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$ with a degree of dissociation $x$,which is small compared with unity. The expression for $K_p$,in terms of $x$ and the total pressure,$P$ is

In a $Victor \ Meyer$ experiment,$0.23 \ g$ of a volatile substance displaces $112 \ mL$ of air at $STP$. Calculate the vapor density of the substance.

For the equations $(i) \ HCN + CCl_4 \rightarrow \alpha_1$ and $(ii) \ HCN + C_6H_6 \rightarrow \alpha_2$,which degree of dissociation is greater,$\alpha_1$ or $\alpha_2$?

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