The equation below represents a chemical reaction at 1 atm and 298 K.
Identify the change in energy that occurs in order to break the bonds in the hydrogen molecules.
2H2 (g) + O2 (g) --> 2H2) (g)
1. Endothermic and absorbed
2. Exothermic and released
3.Endothermic and released
4.Exothermic and absorbed

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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.