Question

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

Answer 1

c) spontaneous

Step-by-step 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 Spontaneous

• ΔG > 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