Consider the following chemical reaction in equilibrium.
CH3COOH
CH3COO-(aq) +H*(aq)
What will happen to the chemical equilibrium if MgCl2 is added?
O
O
The chemical equilibrium of the system will be unaffected.
The chemical equilibrium of the system will shift to the right to favor the forward reaction.
The chemical equilibrium of the system will shift to the left to favor the reverse reaction.
The chemical equilibrium of the system will be damaged irreversibly.
O

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.

Answer///an early form of the atomic theory; dalton atomic theory;

Answerthe same as;