300 ml of a 0.694 m hcl aqueous solution is mixed with 300 ml of 0.347 m ba(oh)2 aqueous solution in a coffee-cup calorimeter. both the solutions have an initial temperature of 28.7 °c. calculate the final temperature of the resulting solution, given the following information: h+(aq) + oh- (aq) → h2o(ℓ) δhrxn = -56.2 kj/mol assume that volumes can be added, that the density of the solution is the same as that of water (1.00 g/ml), and the specific heat of the solution is the same as that for pure water, 4.184 j/(gk).

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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.