Calculate the % impurity in a 0.7 gm of Na2CO3 impure sample that required of O. IN HCI standard solution 30 ml, Atomic mass Na:23,C:12,0:16​

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.

It's called the falling actionwrong subject by the way

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Looking up graphs on google, you can see thaty = force(n)x = time(s)