A 0.10 mol sample of solid zinc was added to 500.0 mL of 1.0 M Cu(NO₃)₂(aq). After the mixture sits overnight, which of the following best describes what was most likely observed and measured the next morning and why?

a) Virtually all of the Zn(s) will have disappeared, and the solution will turn blue due to the presence of excess Cu(NO₃)₂(aq).
b) No observable change would be noticed because zinc does not react with copper nitrate under normal conditions.
c) The solution will become cloudy due to the formation of insoluble zinc nitrate precipitate.
d) Virtually all of the Zn(s) will have disappeared, and Cu(s) will have appeared in the beaker because the reaction went almost to completion at equilibrium due to the very large Keq.