Think about the lab procedure you just read. Label
each factor below with V for "variable" or C for
"constant"
The temperature of the gas:
The amount of gas in the tube (in terms of mass
and moles): 1
The radius of the tube:
The temperature of the gas (changed by the water
surrounding it): Y
The type of gas:
The pressure of the gas:

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.