ElectrochemistryHard
Question
EMF of the cell: Cd(s)|CdCl2.5H2O (sat.)|AgCl(s)|Ag(s) is +0.70 V at 0°C and +0.60 V at 50°C. If ΔHo and ΔSo are temperature independent, then the correct information(s) regarding the cell reaction is/are
Options
A.ΔG° = −115.8 kJ at 50°C
B.ΔG° = 135.1 kJ at 0°C
C.ΔS° = −386 J/K
D.ΔH° = −221.178 kJ
Solution
Net cell reaction is
Cd(s) + 2AgCl(s) $\rightleftharpoons$ 2Ag(s) + Cd2+ (aq) + 2Cl– (aq)
ΔGo50°C = −nFE° = −2 × 96500 × 0.6 = −115800 J
ΔGo0°C = −nFE° = −2 × 96500 × 0.7 = −135100 J
$\Delta S^{o} = nF.\left( \frac{E_{2}^{o} - E_{1}^{o}}{T_{2} - T_{1}} \right) = 2 \times 96500 \times \frac{0.6 - 0.7}{50} = - 386\text{ J/K}$
ΔH° = ΔG° + T ⋅ ΔS° = (–135100) + 273 × (–386) = –240478 J
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