For a galvanic cell using Fe | Fe^2+(0.25 M) and Pb | Pb^2+(0.25 M) half-cells,

Question

For a galvanic cell using Fe | Fe^2+(0.25 M) and Pb | Pb^2+(0.25 M) half-cells, which of the following statements is correct? Fe^2+(aq) + 2e^- rightarrow Fe(s); E degree =-0.41 V Pb^2+(aq) + 2e^- rightarrow Pb(s); E degree =-0.13 V The iron electrode is the cathode When the cell has completely discharged, the concentration of Pb^2+ is zero The mass of the iron electrode increases during discharge The concentration of Pb^2+ decreases during discharge Electrons leave the lead electrode to pass through the external circuit during discharge

Explanation / Answer

the most negative will oxidize, that is, Fe

then

a. is false, since iron must be in teha node (oxidation)

b. false, when this is true, all will be Pb+2 = 0

c. false, since Fe+2 is formed FROM Fe(s) then mass goes to aquous ion

d. True, since it forms Pb(s)

e. false, electrons go from anode to cathode

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