In: Chemistry
1) Calculate the standard potential (Eo value) for the following redox reaction.
2) Circle the reducing agent.
2NO3–(aq) + 8H+(aq) + 3Cu(s) 2NO(g) + 4H2O(l) + 3Cu2+(aq)
Eo =
NO3–(aq) + 4 H+(aq) + 3 e– NO(g) + 2 H2O E0= +0.96 ----------(1)
Cu2+(aq) + 2 e– Cu(s) E0= +0.34 ----------(2)
Cu(s)Cu2+(aq) + 2 e– E0= -0.34 ----------(3)
(1)x2 + (3)x3 2NO3–(aq) + 8H+(aq) + 3Cu(s) 2NO(g) + 4H2O(l) + 3Cu2+(aq)
the standard potential E0= 2x0.96 + 3x(-0.34) = 1.92-1.02 =0.90 V
The reducing agent is Cu(s) as it reduces NO3– to NO