Which is the correct expression for the h-atom balance for the reaction below occurring at steady state with a feed flow rate of 100 mol/s that is equimolar ch4 (a) and o2 (b)? ch4 + o2hcho + h20 assume that the conversion of reaction is 100%. select one: o a. 50 mol/s = 2nhcho + 2nh20 - 4nch4 o b. 50 mol/s = 4nch4 + nhcho + 2nh20 o c. 200 mol/s = 2nch4 + nhcho + 3nh20 o d. 200 mol/s = 2nhcho + 2nh20 o e. not enough information is given

Abbreviated as mg-25.

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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.