For a voltaic cell whose two half-cells are 1.0 M Fe^2+ with an iron (Fe) electr

Question

For a voltaic cell whose two half-cells are 1.0 M Fe^2+ with an iron (Fe) electrode and 1.0 M2n^2+ with a zinc [Zn] electrode, which ONE of the following statements is correct? The standard reduction potentials are Fe^2+(aq) + 2e^- rightarrow Fe(s); Edegree = -0.41 V Zn^2+(aq) + 2e^- rightarrow Zn(s); Edegree = -0.76 V A) The iron electrode is the anode. B) The concentration of Fe^2+ decreases during discharge. C) The mass of the zinc electrode increases during discharge. D) The concentration of Zn^2+ decreases during discharge. E) Electrons leave the iron electrode to pass through the external circuit during discharge. 22. The Faraday constant is defined as- A) The charge per mole of electrons. B) The charge on a single electron. C) The maximum work obtainable from an electrochemical cell. D) The electromotive force of the cell. E) The amount of charge moved between electrodes. 23. Given: Pb^2+(Aq) + 2e^- pB(S); eDEGREE = -0.13 V Mg^2+(aq) + 2e^- mg(s); Edegree = -2.38 V Ag^+(aq) + e^- Ag(s); Edegree = 0.80 V 2H^+(aq) + 2e^- H_2(g); Edegree = 0.00 V Under standard-state conditions, which of the following is the best reducing agent? A) H_2 B) Mg^2+ C) Ag^+ D) Pb E) Ag

Explanation / Answer

21.

Apply

E°cell = Ered - Eox

note that for a spotnanus reactn, E°cell must be positive

so

Ered > Eoxalways

then

E Fe+2 is reduced and Zn+2 will oxidize

all oxidation will decrease in mass; since they will go into aquous solution,

all reduction increases mass, since aquous ions go to deposit as solid material.

A; can't be since it is being reduced, reduction goe sto cathode

B:Fe+2 ions decrease, since they form solid Fe(s)

C:False, it will decrease since it form sions

D: False, Zn+2 ions increases since mass of solid forms ions

E:False, they go TO the iron electrode

choose B

NOTE Consider posting multiple questions in mutliple set of Q&A.

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