1. Briefly explain why we expect to see the mass go up as the iron undergoes a reaction in this experiment.2. Magnesium undergoes a similar reaction with oxygen. Write the balanced chemical equation for the reaction between magnesium and oxygen gas. 3. Consider a reaction where 0.432 g of magnesium ribbon undergoes the above reaction to make 0.745 g of magnesium oxide as a product. How many moles of magnesium are in the final product? How many moles of oxygen?

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.

Pretty sure it's d. heterogeneous is separated by physical properties.