In the activity, click on the E∘cell and Keq quantities to observe how they are related. Use this relation to calculate Keq for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occur in the cell are

Cu2+(aq)+2e−→Cu(s) and Co(s)→Co2+(aq)+2e−

The net reaction is

Cu2+(aq)+Co(s)→Cu(s)+Co2+(aq)

Use the given standard reduction potentials in your calculation as appropriate. ( Keq=5.88*10^20)

In the activity, click on the Keq and ΔG∘ quantities to observe how they are related.

Calculate ΔG∘ using this relationship and the equilibrium constant (Keq) obtained in Part A at T=298K: Keq=5.88*10^20