In Part B you calculated ΔG∘ for the following redox reaction:Cu2 + (aq) + Co (s) →Cu (s) + Co2 + (aq), ΔG∘=-1.18*105JBased on the value of ΔG∘ for the given redox reaction, identify the spontaneity of the reaction. a) nonspontaneousb) at equilibriumc) spontaneous

c) spontaneous

Explanation:

According the equation of Gibb's free energy -

∆G = ∆H - T∆S

∆G = is the change in gibb's free energy

∆H = is the change in enthalpy

T = temperature

∆S = is the change in entropy.

And, the sign of the ΔG, determines whether the reaction is Spontaneous or non Spontaneous or at equilibrium,

i. e.,

if

ΔG <0, the reaction is SpontaneousΔG> 0, the reaction is non Spontaneous ΔG = 0, the reaction is at equilibrium

From the question,

The value for ΔG is negative,

Hence,

ΔG < 0, the reaction is Spontaneous