A gas occupying a volume of 725 mL at a pressure 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume?
a. 725 mL
c. 2470 mL
b. 404 mL
d. 1300 mL

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.

A)  it is neutral because the concentration of hydronium ions equals that of hydroxide ions