Complete the product side of the following net ionic redox equations. Consult the attached activity series table. Make sure the equations are balanced. Indicate states. Write “no reaction” or “N. R.” if the reaction does
not occur.
Ca (s) + Ni2+ (aq)-
Pt (s) + 2 H(aq) -
H2(g) + Cu2+ (aq)-
2 Ag (s) + Pb2+ (aq)-

Answerstrong acids and bases completely dissociate in water.this is how strong acids and bases are defined. they will ionize 100% in solution, making a non-reversible reaction

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.

The image seems to be behind the mirror, but nothing is really there.just took the test.