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Electrode potentials and electrochemical cells (A-level only)

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Question 12

The theoretical EMF of a hydrazine–oxygen fuel cell operating under alkaline conditions is +1.56 V+1.56\text{ V}+1.56 V.

The standard electrode potential for one of the electrodes in this cell is:

N2(g)+4H2O(l)+4e−→N2H4(aq)+4OH−(aq)E⊖=−1.16 V \text{N}_2\text{(g)} + 4\text{H}_2\text{O(l)} + 4\text{e}^- \rightarrow \text{N}_2\text{H}_4\text{(aq)} + 4\text{OH}^-\text{(aq)} \quad E^\ominus = -1.16\text{ V} N2​(g)+4H2​O(l)+4e−→N2​H4​(aq)+4OH−(aq)E⊖=−1.16 V

Give the half-equation for the other electrode and calculate its standard electrode potential.

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

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