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.......$\%$

For the equilibrium reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the value of $K_p$ is $2$. Calculate the percentage dissociation of $N_2O_{4(g)}$ at a total pressure of $0.5 \ atm$. (in $\%$)

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.

The vapour density of $PCl_5$ is $104.16$,but when heated to $230 \, ^\circ C$,its vapour density decreases to $62$. What is the degree of dissociation of $PCl_5$ at this temperature (in $\%$) ?

In a closed vessel,the dissociation of phosphorus pentachloride occurs as: $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$. If the total pressure at equilibrium is $P$ and the degree of dissociation of $PCl_5$ is $x$,then the partial pressure of $PCl_3$ will be:

The degree of dissociation of a weak acid is $7.2 \times 10^{-4}$. What is the value of its percent dissociation in a $0.025 \ M$ solution (in $\%$)?