The actual yield of a product in a reaction was measured as 1.20g. If the theoretical yield of the reaction is 1.82g, What is the percentage yield of the product? A. 65.9%
B. 67.2%
C. 71.9%
D. 73 3%

Because a model would make the investigation easier to understand

The correct answer is:   bri hope this answer was ! : )

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.