In a quiz I got a reaction, not thermodynamically favorable: Cu₂S → 2Cu(s) + S(s) ∆G°...

Question

Question

In a quiz I got a reaction, not thermodynamically favorable:

Cu₂S → 2Cu(s) + S(s) ∆G° = + 86kJ/mol

The question said: 'We can force this to happen by using a battery'..

(i) Using ∆G°, calculate E°cell

....

They then gave the reduction potential of Cu, and put the reduction reaction of sulfur with unknown reduction potential

Cu2+ + 2e- → Cu E° = 0.34
S + 2e- → S2- E°= ???

(ii) Using your answer in part (i), calculate the reduction potential of sulfur in the table

....

\\\ Please clarify with steps, I hope I didn't forget some given info. If I did, lmk. But that's most likely what I got in the exam.

Thanks in advance!

Answer 1

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