How many grams of oxygen are produced in the following reaction when you start with 1.90 moles of water? Assume 100\% yield 2H 2 O 2H 2 +O 2

13) a 14) a15) b16) i don't know sorry17) a (maybe)

Just took the quiz on edgenuity and the correct answer is "c.  4.54 x  10–12  j"

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.