Homework Answers
Answer:
This problem is based on electrochemical cell. The relation between Standard Gibb's Free energy and Cell potential is given as,
Gocell
= - nFEo. ------------ (1)
Given data :
n = # of electtrons transfered in cell reaction = 2 (as shown in cell reaction)
F = Faraday's constant = 96485 C
Eo = -430.0 V
Using these values in eq.(1) we get,
Gocell
= - 2 x 96485 x (-0.430)
Gocell
= + 82977 J
Gocell
= + 82.977 kJ
Standard Gibbs Free energy change for given chemical change at 25.0 oC is +82.977 kJ.
As per spontaneity criteria, the thermochemical change with +ve
Gocell
is non-spontaneous in specified direction.
Hence shown thermochemical transformation is non-spontaneous in specified direction.
According to Nernst equation
Ecell = Eocell -(RT/nF) lnK
I.e. With increase in temperature (RT/nF) lnK value becomes more -ve and hence
Eocell - (RT/nF) lnK tends to be +ve and so the
Gocell
value become -ve which makes the reaction spontaneous above that
temperature.
Hence Temperature of the reaction needed to be increased to make the reaction spontaneous in specified direction.
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