Question 7 Use standard reduction potentials to calculate AG for the reaction: 3 CN + 2...

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Answer 1

Answer #1

Sol :-

Given reaction is :

3CN- + 2MnO4- + H2O -------------------> 3CNO- + 2MnO2 + 2OH-

Oxidation half cell reaction is :

3CN- + 6OH- -----------------> 3CNO- + 3H2O + 6e- , E0oxidation = +0.970 V

Reduction half cell reaction is :

2MnO4- + 4H2O + 6e- -----------------> 2MnO2 + 8OH- + 4H2O , E0reduction = + 0.595 V

Standard cell potential (E0) = E0oxidation + E0reduction

= 0.970 V + 0.595 V

= 1.565 V

Number of electron exchange (n) = 6

The realtionship between E0 and Gibb's free energy change (ΔG0) is :

ΔG0 = -nFE0

= -(6).(96500 C).(1.565 V)

= -906135 J , Because, 1CV = 1 J

= - 906.135 KJ

Hence, ΔG0 = - 906.135 KJ

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Answer 2

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