Same chapter3 marksDifficulty: Medium
Calculate the emf of the cell Zn | Zn2+(1 M) || Cu2+(1 M) | Cu, given E° for Zn2+/Zn = −0.76 V and for Cu2+/Cu = +0.34 V.
Electrochemistry
3 marksDifficulty: Medium
State the Nernst equation for an electrode and explain the terms in it.
Original Khojo Papers practice question — not from a past board paper.
Answer
For the reduction Mn+ + ne− → M the electrode potential is E = E° − (0.0591/n) log(1/[Mn+]) at 298 K, where E° is the standard electrode potential, n the number of electrons transferred and the bracket the molar concentration of the ion.
No citable source has been recorded for this record. Treat it as practice material, not as fact.
Explanation
The equation shows how the potential varies with concentration, which the standard potential alone does not.
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Solutions