Consider the following reaction: 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g)

If 218 g of H2S reacts with excess oxygen, and 94.1 g of water was collected after the reaction has gone to completion, what is the percent yield of the reaction?

Group of answer choices

A)43.2 %

B)46.0%

C)81.6%

D)92.4%
pls explain your answer

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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.