Which of the following is true for a first order reaction? None of the above.

The reaction has a half-life that is independent of initial concentrations.

The rate is independent of concentration.

A plot of concentration of the reactant versus time yields a straight line.

Depends on the speed of the car.

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.

Precipitate, and gas

D. h2o + h2o > h3o + oh- confirmed.