Degree of dissociation of an electrolyte does not depend on

For the following equilibrium $N_2O_4 \rightleftharpoons 2NO_2$ in gaseous phase,$NO_2$ is $50\%$ of the total volume when equilibrium is set up. Hence,the percentage of dissociation of $N_2O_4$ is.......$\%$

The equilibrium constant for the decomposition of $H_2O_{(g)}$: $H_2O_{(g)} \rightleftharpoons H_{2(g)} + \frac{1}{2} O_{2(g)}$ $(\Delta G^{\circ} = 92.34 \ kJ \ mol^{-1})$ is $8.0 \times 10^{-3}$ at $2300 \ K$ and the total pressure at equilibrium is $1 \ bar$. Under this condition,the degree of dissociation $(\alpha)$ of water is $............ \times 10^{-2}$ (nearest integer value). [Assume $\alpha$ is negligible with respect to $1$]

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:

If $PCl_5$ undergoes $80\%$ dissociation at $250 \, ^\circ C$,what is its vapour density at this temperature?

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