Question

Calculating free energy (delta G)

Answer 1

\[\frac{ 1 }{ 2 }Zn ^{2+}(aq)+\frac{ 1 }{ 2 }Cu(s) \rightarrow \frac{ 1 }{ 2 }Zn(s) + \frac{ 1 }{ 2 }Cu ^{2+}(aq)\]

the arrow is reversible, how do i calculate \[DeltaG ^{0} from this reaction? \]

Answer 2

I would use the standard cell potentials for copper and zinc, then use \(\Delta G = -nFE\) since its a redox reaction

Answer 3

but why is the standard cell potential negative? like -3x96484x-1.543= +447 kj/mol is the answer

Answer 4

a negative cell potential tells us that the reaction is not spontaneous. It will not run in the direction written