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

From the question ,

The value for ΔG is negative ,

Hence ,

ΔG < 0 , the reaction is Spontaneous

there are two significant figures.