In a calorimeter 72.55 g of an unknown metal at 71.6 °C is added to 58.85 g of water at 22.4 °C. After stirring and waiting for the system to reach equilibrium, the final temperature reached 47.3 °C. Calculate the specific heat of the metal. (The specific heat of water is 4.184 j/g 0C).

The answer should be c.

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.