Question

Calculate the standard electrode potential for the redox reaction between silver and copper ions at 298K, given that the reduction potential for the half-reaction Ag+ + e- → Ag is +0.80 V and the reduction potential for the half-reaction Cu2+ + 2e- → Cu is +0.34 V.

Answer 1

To calculate the standard electrode potential for the redox reaction between silver and copper ions, we need to determine the overall cell potential. This can be done by subtracting the reduction potential of the anode  the half-reaction that undergoes oxidation  from the reduction potential of the cathode  the half-reaction that undergoes reduction .In this case, we have the following half-reactions:1. Ag+ + e-  Ag  reduction potential = +0.80 V 2. Cu2+ + 2e-  Cu  reduction potential = +0.34 V Since the reduction potential of the silver half-reaction is higher than that of the copper half-reaction, silver will act as the cathode  undergo reduction  and copper will act as the anode  undergo oxidation . Therefore, the copper half-reaction needs to be reversed to represent oxidation:Cu  Cu2+ + 2e-  oxidation potential = -0.34 V Now, we can calculate the overall cell potential:E_cell = E_cathode - E_anodeE_cell =  +0.80 V  -  -0.34 V E_cell = +0.80 V + 0.34 VE_cell = +1.14 VThe standard electrode potential for the redox reaction between silver and copper ions at 298K is +1.14 V.