ElectrochemistryHard
Question
The standard emf of the cell, Cd(s) | CdCl2(aq) (0.1 M) || AgCl(s) | Ag(s) in which the cell reaction is,
Cd(s) + 2AgCl(s) → 2Ag(s) + Cd+2 (aq) + 2Cl-(aq) is 0.6915 V at 0oC and 0.6753 V at 25oC. The ᐃHo of the reaction at 25oC is :
Cd(s) + 2AgCl(s) → 2Ag(s) + Cd+2 (aq) + 2Cl-(aq) is 0.6915 V at 0oC and 0.6753 V at 25oC. The ᐃHo of the reaction at 25oC is :
Options
A.- 176 kJ
B.- 234.7 kJ
C.+ 123.5 kJ
D.- 167.26 kJ
Solution
= -6.48 × 10-4 V deg-1 ᐃH298 = - neF + nFT
= - 2 × 0.6753 × 96500 + 2 × 96500 × 298 × (-6.48 × 10-4)= 2 × 96500 (- 0.6753 - 0.1931) = - 167.6 KJ.
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