Consider the unbalanced reaction Ti(s) + Cl2(g) --> TiCl4(s) When 4.21 g of Ti react with 15.4 g of Cl2, 16.2 g of TiCl4 are obtained. The theoretical yield of TiCl4 is___, the limiting reactant is___and the percent yield is___ %. (Remember to use correct sig figs)

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.