You have a liquid-phase mixture of 0.450 mol fraction ethanol and 0.550 mol fraction water at 760.0 mmHg. You\'d like to calculate the bubble-point temperature of the mixture, and the composition of the vapor formed at the bubble-point temperature two different ways. For the first method, assume that the solution behaves ideally and all components follow Raoult\'s law. What is the bubble-point temperature of the solution?

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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.