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Hg2+ + 2e- --> Hg Eo = 0.85
Zn2+ + 2e----> Zn Eo= -0.76
115. Given the cell potentials shown above, the equilibrium constant at 298 K for the reaction
Zn + Hg2+ --> Zn2+ + Hg
Is closest to which of the following?
My answer would be C. but the answer is A. how?
X+ + e- ---> X(s) Eo= -2.174
11. For the half rxn above, which of the following is a correct statement?
Here we see that X+ is being reduced, yet the Eo shows an oxidizing rxn (because it is negative value), would this be the reason.
My answer is A but the correct ans. is E. how come?
Zn2+ + 2e----> Zn Eo= -0.76
115. Given the cell potentials shown above, the equilibrium constant at 298 K for the reaction
Zn + Hg2+ --> Zn2+ + Hg
Is closest to which of the following?
- 2.5 × 1054
- 54
- 1.6
- 1.8×102-
My answer would be C. but the answer is A. how?
X+ + e- ---> X(s) Eo= -2.174
11. For the half rxn above, which of the following is a correct statement?
- X+ is readily reduced
- X+ is a good oxidizing agent
- X is a poor reducing agent
- X is a good oxidizing agent
- X is readily oxidized
Here we see that X+ is being reduced, yet the Eo shows an oxidizing rxn (because it is negative value), would this be the reason.
My answer is A but the correct ans. is E. how come?
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