Exactly 10.7 mL of water at 28.0 °C is added to a hot iron skillet. All of the water is converted into steam at 100.0°C. The mass of the pan is 1.40 kg and the molar heat capacity of iron is 25.19 J/(mol·°C). What is the temperature change of the skillet?

The change in the temperature of the iron is a decrease of 14.0ºC.

Explanation:

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Sorry i dont understand the question can you rephase it?

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.