What is the oxidizing agent in the redox reaction represented by the following cell notation? Mg( s) ∣ Mg 2+( aq) Cu +( aq) ∣ Cu( s)
Mg(s)
Cu+(aq)
Mg2+(aq)
Pt
Cu(s)

Which of the following is the weakest reducing agent?
Au(s)
OH2(g)
Sn(s)
ClO2-(aq)
Cl⁻(aq)

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It shows that the experiment is designed properly.

The correct answer would be b) volume versus temperature, because they are also directly proportional.

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.