For the reaction $P \rightleftharpoons Q + R$,initially $2 \, \text{mol}$ of $P$ is taken. At equilibrium,$0.5 \, \text{mol}$ of $P$ dissociates. The degree of dissociation will be ...... .

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).

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 $1$]

The vapour density of $N_2O_4$ in the equilibrium $N_2O_4 \rightleftharpoons 2NO_2$ is $40$. The degree of dissociation is:

The vapour density of a gas is $11.2$. The volume occupied by $11.2 \ g$ of the gas at $STP$ will be.....$L$

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 $\%$) ?