Total number of moles for the reaction $2HI \rightleftharpoons H_2 + I_2$ at equilibrium,if $\alpha$ is the degree of dissociation,is:

At temperature $T$,the dissociation equilibrium of $AB_{2(g)}$ is given as: $2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$. If the degree of dissociation $x$ is very small compared to $1$,then the expression for the equilibrium constant $K_p$ in terms of $x$ and total pressure $P$ is:

For the equilibrium $PCl_{5_{(g)}} \rightleftharpoons PCl_{3_{(g)}} + Cl_{2_{(g)}}$,the observed vapour density of the mixture is $80$. Given atomic masses $P = 31$ and $Cl = 35.5$,the degree of dissociation of $PCl_{5_{(g)}}$ is approximately....$\%$

Which of the following will have the highest degree of dissociation for $4-$nitrophenol in an aqueous solution (in $M$)?

Ammonium carbamate $(NH_4COONH_2)$ when heated to $200 \ ^oC$ gives a mixture of $NH_3$ and $CO_2$ with a vapour density of $26$ at equilibrium. What is the degree of dissociation of ammonium carbamate?

If the vapor density of a volatile substance relative to $CH_4$ is $4$,then find the molecular mass of that substance.