In the electrochemistry lab we assumed that the electrode process at the copper
ID: 1019963 • Letter: I
Question
In the electrochemistry lab we assumed that the electrode process at the copper cathode in the sulfuric acid solution was 100% efficient and no other reactions were taking place at this electrode cathode. What if water was reduced at the copper-wire cathode as well as the hydrogen ions? 2H20 + 2e- ---> H2 (g) + 2OH - (aq). What affect would this have on the calculated value of the equivalent mass for the unknown metal (increase, decrease, or remain the same). Explain/give reasoning for your answer. *EDIT: Ered = -0.83 2H2O (l) + 2e- ---> H2(g) + 2OH- (aq) , Ered = 0.34 Cu2 (aq) + 2e- ---> Cu (s),
Explanation / Answer
As the reduction potential values provided only copper ion undergoes reduction but not water because its reduction potential is smaller than that of copper.
Incase, if water is reduced at copper wire, the equivalent mass copper would decrease as it undergoes oxidation simultaneously.