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Electrode potentials and electrochemical cells (A-level only)

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Question 10

Some electrode potential data are shown:

Fe2+(aq)+2e−→Fe(s)E⊖=−0.44 VAg+(aq)+e−→Ag(s)E⊖=+0.80 V \begin{aligned} \text{Fe}^{2+}(\text{aq}) + 2\text{e}^- &\rightarrow \text{Fe}(\text{s}) \quad E^\ominus = -0.44\text{ V} \\ \text{Ag}^+(\text{aq}) + \text{e}^- &\rightarrow \text{Ag}(\text{s}) \quad E^\ominus = +0.80\text{ V} \end{aligned} Fe2+(aq)+2e−Ag+(aq)+e−​→Fe(s)E⊖=−0.44 V→Ag(s)E⊖=+0.80 V​

Which is a correct statement about this cell?

Fe(s)∣Fe2+(aq)∥Ag+(aq)∣Ag(s) \text{Fe}(\text{s}) \mid \text{Fe}^{2+}(\text{aq}) \parallel \text{Ag}^+(\text{aq}) \mid \text{Ag}(\text{s}) Fe(s)∣Fe2+(aq)∥Ag+(aq)∣Ag(s)

Electrons travel in the external circuit from iron to silver.

The concentration of silver(I) ions increases.

The standard EMF of the cell is 0.36 V0.36\text{ V}0.36 V.

Iron is deposited.

Electrode potentials and electrochemical cells (A-level only) Questions

  1. A Level
  2. /Chemistry
  3. /Electrode potentials and electrochemical cells (A-level only)