Imix 6.00 g of ki and 8.00 g of i2in 0.500 l of water and hook this up with a saltbridge to a mixture of 4.00 g of clo2and 7.00 g of kclo2in a separate beaker with 0.500 l ofwater. if 2 a of current is allowed to pass through the circuit for 10 minutes, what would the final cell potential be? i2(s) + 2 e-2 i-(aq) e0 red = 0.54 v2 clo2(aq) + 2 e-2 clo2-(g) e0red= 0.95 v

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.

The answer you are looking for is option d

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