Calculate the standard cell potentials of galvanic cell in which the following reactions take place:
Fe2+ (aq) + Ag+ (aq) → Fe3+(aq) + Ag(s)
Calculate the ΔrG° and equilibrium constant of the reaction.
The galvanic cell of the given reaction is represented as
Fe2+(aq) | Fe3+(aq) || Ag+ | Ag(s)
The formula of standard cell potential is
Eocell = Eo right – Eoleft
Eocell = 0.80 – 0.77
Eocell = + 0.03 V
In balanced reaction there are 1 electron are transferring so that n = 1
Faraday constant, F = 96500 C mol−1
Eocell = + 0.03 V
Use formula
∆rGθ = – nFEocell
Plug the value we get
Then, = −1 × 96500 C mol−1 × 0.03 V
= −2895 CV mol−1
= −2895J mol−1
= −2.895 kJ mol−1
Again,
Use second formula of ∆rGθ
∆rGθ = −2.303RT log kC
log KC = (∆rGθ) /( – 2.303RT)
plug the values we get
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