When zinc metal reacts with oxygen gas, 2Zn(s) + O2(g) → 2ZnO(g) large amounts of light and heat are released. A student states that this reaction is a combustion reaction but not a redox reaction. Do you agree? Defend your answer by explaining whether or not it meets the requirements of each type of reaction

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.

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H tricky one let me think and get back to u