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Redox and electrode potentials

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Question 2

An electrochemical cell is constructed from the two standard redox systems below:

Ni2+(aq)+2e−⇌Ni(s)E⊖=−0.25 V \text{Ni}^{2+}(\text{aq}) + 2\text{e}^- \rightleftharpoons \text{Ni}(\text{s}) \quad E^{\ominus} = -0.25\text{ V} Ni2+(aq)+2e−⇌Ni(s)E⊖=−0.25 V Ag+(aq)+e−⇌Ag(s)E⊖=+0.80 V \text{Ag}^+(\text{aq}) + \text{e}^- \rightleftharpoons \text{Ag}(\text{s}) \quad E^{\ominus} = +0.80\text{ V} Ag+(aq)+e−⇌Ag(s)E⊖=+0.80 V

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

  1. The standard cell potential is 1.05 V.
  2. The reaction occurring at the nickel electrode is Ni2+(aq)+2e−→Ni(s)\text{Ni}^{2+}(\text{aq}) + 2\text{e}^- \rightarrow \text{Ni}(\text{s})Ni2+(aq)+2e−→Ni(s).
  3. The mass of the nickel electrode decreases as the cell operates.

1, 2 and 3

Only 1 and 3

Only 2 and 3

Only 1

Redox and electrode potentials Questions

  1. A Level
  2. /Chemistry
  3. /Redox and electrode potentials