ElectrochemistryHard
Question
The efficiency of an hypothetical cell is about 84% which involves the following reaction :
A (s) + B2+ (aq) → A2+ (aq) + B (s) : ᐃH = - 285 kJ
Then, the standard electrode potential of the cell will be (Assume as ᐃS = 0)
A (s) + B2+ (aq) → A2+ (aq) + B (s) : ᐃH = - 285 kJ
Then, the standard electrode potential of the cell will be (Assume as ᐃS = 0)
Options
A.1.20
B.2.40 V
C.1.10 V
D.1.24 V
Solution
A(s) +B2+aq. → Aaq.2+ + B(s) , ᐃHo = - 285 KJ
Assuming ᐃs to negligible, ᐃGo = ᐃHo = - 285 × 103 × 0.84 = - 2 × Eo × 96500
Eo = 1.24 Volt
Assuming ᐃs to negligible, ᐃGo = ᐃHo = - 285 × 103 × 0.84 = - 2 × Eo × 96500
Eo = 1.24 Volt
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