2. In the reaction H2(g) + b(0) + 2HI(), there are equilibrium partial pressures of PH, = 13.0 MPa, P = 11.7 MPa and Phi = 66.6 MPa. What is the
equilibrium constant K, for this reaction?
O A 0.44
B.228
OC.143
D. 292

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.