Of the test tubes pictured below, which one will have the slowest reaction rate with a piece of magnesium metal? Explain why.
1 M
0.01 M
HCl(aq)
HCl(aq)
1.
3.
10 mL
110 mL
0.001 M
0.1 M
HCl(aq)
HCl(aq)
2.
10 mL
10 mL

D)can be increased in a closed system

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.

The correct answer to this question is 28