If 3.500 moles of water react completely according to the following equation, how much heat must be absorbed in kilojoules? 6CO2+6H2O⟶C6H12O6+6O2 ΔH=2,803 kJ Your answer should have four significant figures (round your answer to a whole number).

Neither model is able to show the reactivity of potassium.

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.

Answer( precipitate );