Answer:
ΔG° = - 27627.1 Joules
ΔE° = 0.290 V
Explanation:
We have to apply the values in two formulas, for ΔG° and ΔE°
ΔG° = - R . T . lnK
ΔE° = 0.06 / n . log K
where T is absolute T°
R is the Ideal Constant Gases
K is Equilibrium constant.
n is the number of e⁻ gained or released during the redox
ΔG° = - R . T . lnK
ΔG° = - 8.31 J/K . 298K . ln 7x10⁴
ΔG° = - 27627.1 Joules
This reaction is spontaneous
ΔE° = 0.06 / 1 . log 7x10⁴
n = 1
ΔE° = 0.290 V
