Calculate the degree of dissociation $\alpha$ for $0.1 \, N \, CH_3COOH$ (dissociation constant $K_a = 1 \times 10^{-5}$).

The vapour density of $PCl_5$ at $25^{\circ}C$ is $100$. Calculate the degree of dissociation at this temperature.

Which of the following equations is correct for the vapour density of completely dissociated ammonium chloride?

Gaseous $N_2O_4$ dissociates into gaseous $NO_2$ according to the reaction:
$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$
At $300 \ K$ and $1 \ atm$ pressure,the degree of dissociation of $N_2O_4$ is $0.2$. If one mole of $N_2O_4$ gas is contained in a vessel,then the density of the equilibrium mixture is.......$g/L$

The vapour density of a mixture containing $NO_2$ and $N_2O_4$ is $27.6$. The mole fraction of $N_2O_4$ in the mixture is

If $D_T$ and $D_0$ are the theoretical and observed vapour densities at a definite temperature and $\alpha$ is the degree of dissociation of a substance,then $\alpha$ in terms of $D_0, D_T$ and $n$ (number of moles of product formed from $1 \, \text{mole}$ of reactant) is calculated by the formula: