Electrochemical cells Flashcards

1
Q

an electrochemical cell is a device used

A

for producing an electric current from chemical reactions

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2
Q
which of the following will be the negative electrode of the cell:
Zn2+(aq) + 2e- ⇌ Zn(s)
E⦵ = -0.76V
Cu2+(aq) + 2e- ⇌ Cu(s)
E⦵ = +0.34V
A

Zn2+(aq) + 2e- ⇌ Zn(s)
E⦵ = -0.76V
Cu2+(aq) + 2e- ⇌ Cu(s)
E⦵ = +0.34V

the E⦵ value for the Zn2+ | Zn half-cell is more negative, so the zinc electrode will be the negative electrode of the cell
so the electrons will flow from the zinc electrode to the copper electrode

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3
Q

the conventions for shorthand notation of representing two half cells in a cell diagram are:

A
  • the two reduced forms of the species are shown on the outside of the cell diagram
  • the positive electrode is shown on the right-hand side of the cell diagram
  • the standard hydrogen electrode is always written on the left-hand side
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4
Q
the cell-diagram for the cell formed by combining the half cells below are:
Zn2+(aq) + 2e- ⇌ Zn(s)
E⦵ = -0.76V
Cu2+(aq) + 2e- ⇌ Cu(s)
E⦵ = +0.34V
A

Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s)

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