Calculate the calorimeter constant of 2.0 g of C2H2(g) were ignited in a 2725g H2O calorimeter and a 4.7deg C temp change was observed. The heat of combustion of C2H2(g) is -1229.5 Kj/Mol.

1= c 2= a or d3 = idk sorry 4= c5= 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.