For the reaction $A \rightleftharpoons nB$,if $a$ moles of $A$ are taken initially and $x$ moles of $A$ dissociate at equilibrium,find the value of the degree of dissociation.

What is the vapor density of a mixture containing $20\%\, NO_2$ by volume and $N_2O_4$?

For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the correct relation between degree of dissociation $(\alpha)$ of $N_2O_{4(g)}$ and equilibrium constant,$K_p$ is $(P=$ total pressure of mixture $)$

Ammonia is heated in a closed vessel in the presence of a catalyst at $15 \ atm$ pressure and a temperature range of $27 \ ^\circ C$ to $347 \ ^\circ C$. Under these conditions,ammonia undergoes partial dissociation according to the reaction $2NH_3 \rightleftharpoons N_2 + 3H_2$. When the pressure is increased to $50 \ atm$ while keeping the volume of the vessel constant,calculate the percentage of $NH_3$ dissociated.

For a $10^{-2} \ M \ HCN$ solution with $[H^+] = 10^{-3} \ M$,find the value of the degree of dissociation in percentage. (in $\%$)

In a $100 \ L$ vessel,$3 \ moles$ of nitrogen and $3 \ moles$ of $PCl_5$ are taken and heated to $500 \ K$. The equilibrium pressure is $3.28 \ atm$. The percentage degree of dissociation of $PCl_5$ is : (Assume ideal behaviour for all gases).