4. A container holds 500 mL of oxygen gas at a pressure of 1.3 atmn and a temperature of 25 "C. If the temperature increases to 22 °C and the pressure increases to 2.0 atm, will the volume of the
gas increase or decrease? What is the final volume of the gas in liters (L)?

Ithink it’s one of those things that you put the object on

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.

Ithink the correct answer is the secned option

This is the whole balanced equation 2bf3 + 3li2so3 --> b2(so3)3 + 6lif