Please help me A certain gas has a volume of 500.0 mL at 77.00C and 600.0 torr. Calculate the temperature, C, if the
volume decreased to 400.0 mL and the pressure is increased to 1.00 atm.

Bthats what im doing to and i figured it out it is b

Here is the link to the all information u need i mean answer key

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.