Chemistry - Thermochemistry Question with Solution | TestHub

(A) Relation: $\Delta S=nF\frac{d{E}_{cell}}{dT}$

Given: $\frac{d{E}_{cell}}{dT}=\frac{2R}{3F}$, $n=3$

Calculate: $\Delta S=3F\times \frac{2R}{3F}=2R\ne 4R$ → A is false

(B) Cell: Pt | H₂ (1 bar) | H⁺ (0.1 M) || H⁺ (0.01 M) | H₂ (1 bar) | Pt

H⁺ moves from 0.1 M → 0.01 M → system becomes less ordered in solution, but because entropy depends on the number of accessible microstates, dissolution of H⁺ lowers concentration → $\Delta S<0$ → B is false

(C) Racemization converts one enantiomer → racemic mixture → disorder increases → $\Delta S>0$

(D) $[CoC{l}_6{]}^{4-}+3en\to [Co(en{)}_3{]}^{2+}+6C{l}^{-}$. This reaction leads to more ions and more disorder → $\Delta S>0$