Consider the reaction. 2 upper N upper o upper c l double-headed arrow 2 upper N upper O (g) plus upper C l subscript 2 (g).

At equilibrium, the concentrations are as follows.

[NOCl] = 1.4 ´ 10–2 M
[NO] = 1.2 ´ 10–3 M
[Cl2] = 2.2 ´ 10–3 M

What is the value of Keq for the reaction expressed in scientific notation?
1.6 ´ 10–5
6.2 ´ 10–4
6.2 ´ 104
1.6 ´ 105

6because i no yea yea

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.