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Question 35

A cell is constructed from the two redox systems below.

Zn2+(aq)+2e−⇌Zn(s)E⊖=−0.76 V \text{Zn}^{2+}(\text{aq}) + 2\text{e}^- \rightleftharpoons \text{Zn}(\text{s}) \quad E^{\ominus} = -0.76\text{ V} Zn2+(aq)+2e−⇌Zn(s)E⊖=−0.76 V Cu2+(aq)+2e−⇌Cu(s)E⊖=+0.34 V \text{Cu}^{2+}(\text{aq}) + 2\text{e}^- \rightleftharpoons \text{Cu}(\text{s}) \quad E^{\ominus} = +0.34\text{ V} Cu2+(aq)+2e−⇌Cu(s)E⊖=+0.34 V

Which statement(s) is/are correct for the cell?

  1. The cell potential is 0.42 V.
  2. The reaction at the zinc electrode is Zn(s)→Zn2+(aq)+2e−\text{Zn}(\text{s}) \rightarrow \text{Zn}^{2+}(\text{aq}) + 2\text{e}^-Zn(s)→Zn2+(aq)+2e−.
  3. The copper electrode increases in mass.

1, 2 and 3

Only 1 and 2

Only 2 and 3

Only 1

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