In which of the following reactions will kc = kp? in which of the following reactions will kc = kp?
(a) so3(g) + no(g) ↔ so2(g) + no2(g)
(b) 2 n2(g) + o2(g) ↔ 2 n2o(g)
(c) 4 nh3(g) + 3 o2(g) ↔ 2 n2(g) + 6 h2o(g)
(d) 2 so2(g) + o2(g) ↔ 2 so3(g)
(e) none of the above reactions have kc = kp.

Answerthe half-reaction having the greatest tendency to occur at the anode:     i₂(aq) + 2e⁻  ⇄ 2i⁻  ;   e = +0.53 v======oxidation occurs at the anode. we must therefore find the half-reaction with the greatest tendency to oxidize.the given values of e are reduction potentials (the form of the half-reactions are of reduction).the lower the reduction potential, the higher the potential to oxidize. the half-cell with the lowest reduction potential will have the greatest tendency to oxidize at the anode.the half-reaction having the greatest tendency must be    i₂(aq) + 2e⁻  ⇄ 2i⁻    e = +0.53 vbecause its reduction potential is the lowest out of the three.