Chemistry - Electrochemistry Question with Solution | TestHub

ChemistryElectrochemistryGalvanic cells/Nernst Equation/Concentration CellsMedium2 minPYQ_2003

ChemistryMediumstatement

For the redox reaction $Zn (s) + Cu^{2 +} (0.1 M) \to Zn^{2 +} (1 M) + Cu (s)$ taking place in a cell, $E_{cell}^{0}$ is $1.10$ volt. $E^{\circ}$ for the cell will be $(2.303 \frac{RT}{F} = 0.0591)$

Options:

Answer:

Solution:

$E_{cell} = E_{cell}^{0} + \frac{0.059}{n} lo g [\frac{Cu ^{+ 2}}{Zn ^{+ 2}}]$ $= 1.10 + \frac{0.059}{2} lo g [0.1] = 1.10 - 0.0295 = 1.07 V$

Stream:JEESubject:ChemistryTopic:ElectrochemistrySubtopic:Galvanic cells/Nernst Equation/Concentration Cells

⏱ 2mℹ️ Source: PYQ_2003

Doubts & Discussion

Loading discussions...