Calculate the percent yield of hydrogen (H2). When going into the lab, 5.00 mols of ammonia (NH3) is decomposed into hydrogen and nitrogen according to the reaction: 2NH3-N2 + 3H2
After the experiment, it is measured that 105.25 L of hydrogen gas was actually recovered. No links please!!

Do you have any options?

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.