For the equations (i) HCN + CCl_4 rightarrow | vedclass

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(B) The degree of dissociation $(\alpha)$ depends on the dielectric constant of the solvent. Higher dielectric constant facilitates greater dissociati

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$\alpha_2 > \alpha_1$

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(B) The degree of dissociation $(\alpha)$ depends on the dielectric constant of the solvent. Higher dielectric constant facilitates greater dissociation of the solute.$CCl_4$ is a non-polar solvent with a dielectric constant of approximately $2.2$.$C_6H_6$ (benzene) is also a non-polar solvent with a dielectric constant of approximately $2.3$.Since the dielectric constant of $C_6H_6$ $(2.3)$ is slightly higher than that of $CCl_4$ $(2.2)$,it facilitates a greater degree of dissociation for $HCN$.Therefore,$\alpha_2 > \alpha_1$.

For the equations $(i) \ HCN + CCl_4 \rightarrow \alpha_1$ and $(ii) \ HCN + C_6H_6 \rightarrow \alpha_2$,which degree of dissociation is greater,$\alpha_1$ or $\alpha_2$?

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