A 350 g iron pot is heated on a stove for a period of time until it is hot. The stove is turned off and 500 g of cold water (12.2 *C) is added to the pot. When the thermal equilibrium is reached, the temperature of water is 29.4*C What was the initial temperature of the iron pot, assuming heat was exchanged between these two objects and none was lost to the surroundings?

I'm not sure but i will try to find out

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.

Answeropposite;