Please, solve question 10. Consider the oxidation(corrosion) of copper metal to
ID: 994352 • Letter: P
Question
Please, solve question 10.
Consider the oxidation(corrosion) of copper metal to Cu^2+ in acid. The two relevant half reactions and reduction potential are given below. i) O_2(aq) + 4H^-(aq) + 4e^+ rightarrow 2H_2O(l) +1.23 V ii) Cu^2+(aq) + 2e^+ rightarrow Cu(s) +0.337V A) Write out the total balanced redox reaction. B) Calculate the total cell potential(E_cell) C) Is this reaction spontaneous? D) Calculate DeltaG of this reaction using DeltaG = n F E_cell where n is the number of e transgerred. F is Faraday's constant and E_cell calculated in part B. 9. Aluminum can also be oxidized in the presence of acid. This half reaction and reduction potential are given below: iii) Al^3+(aq) + 3e^- rightarrow Al(s) -1.66 V A) Calculate the cell potential for the correction of aluminum in acid (half reactions (i) and (iii)). B) Calculate DeltaG. 10) Comparing your answer to question 8 and 9 if both Al and Cu are present in an acidic aqueous solution, which species will be osidized first?Explanation / Answer
From electrode potential of two metals,
Aluminium has Eel = -1.66 V
Copper has Eel = +0.337 V
An electrode with greater negative value, the greater tendency to get oxidized. So, Aluminium oxidizes first.
Don't forget these are two different cells.
For your knowledge, when an aluminium foil is placed in aq.CuCl2.2H2O solution. Cu get reduced by aluminium and Cu metal deposits on Al foil. It shows the great oxidizing property of Al than Cu.