What is the TOTAL ionic equations for the following? Ca(ClO)2(aq) + 4HCl(aq) --> CaCl2(aq) + 2H2O(l) + 2Cl2(g)

SrBr2(aq) + K2SO4 (aq) --> SrSO4 (s) + 2 KBr (aq)

2 Cr(NO3)3 (aq) + 3 FeSO4 (aq) --> 3 Fe(NO3)2 (aq) + Cr2(SO4)3 (aq)

Bar graph

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.