Chemistry - Electrochemistry Question with Solution | TestHub

Question Explanation:

Which of the following is/are correct for the disproportionation reaction.

Concept:

This question is based on feasibility of disproportionation reaction.

Solution:

Disproportionation:

1.${\mathrm{E}}_{\text{cell }}^{\circ }={\mathrm{E}}_{\text{red }}^{\circ }-{\mathrm{E}}_{\text{ox }}^{\circ }={\mathrm{E}}^{\circ }\left({\mathrm{TI}}^{+}/\mathrm{TI}\right)-{\mathrm{E}}^{\circ }\left({\mathrm{TI}}^{3+}/{\mathrm{TI}}^{+}\right)=-0.34-1.25=-1.59\mathrm{V}$. Highly non1. spontaneous. (1) is correct.

2. $3{\mathrm{E}}^{\circ }\left({\mathrm{TI}}^{3+}/\mathrm{TI}\right)=2\left(1.25\right)+1\left(-0.34\right)=2.50-0.34=2.16\Rightarrow {\mathrm{E}}^{\circ }=0.72V$(2) is correct.

3. ${\mathrm{E}}^{\circ }\left({\mathrm{TI}}^{3+}/{\mathrm{TI}}^{+}\right)=1.25V>1.23V$ of O₂ . (3) is correct.

4. Complexing the product of disproportionation (Tl³⁺ ) shifts the equilibrium to the right. (4) is correct.