A galvanic cell consists of a metallic zinc plate immersed in 0-1 M ZnNO32 solution- Calculate the emf of the cell at 25-C- Write the chemical equations for the electrode reactions and represent the cell- Given- EZn2- Zn- - -0-76 volt and EPb2- Pb- - -0-13 volt-

E_cell=0.76 0.13=0.63V E_cell=E^∘ RTnFlnQ ...

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Standard XII

Chemistry

EMF

A galvanic ce...

Question

A galvanic cell consists of a metallic zinc plate immersed in $0.1 M Z n (N O_{3})_{2}$ solution. Calculate the emf of the cell at $25^{\circ} C$ . Write the chemical equations for the electrode reactions and represent the cell. (Given: $E_{Z n^{2 +} / Z n}^{\circ} = - 0.76 v o l t$ and $E_{P b^{2 +} / P b}^{\circ} = - 0.13 v o l t$ .

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Solution

$E_{c e l l} = 0.76 - 0.13 = 0.63 V$
$E_{c e l l} = E^{\circ} - \frac{R T}{n F} l n Q$

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A galvanic cell consists of a metallic zinc plate immersed in 0.1 M Zn(NO3)2 solution. Calculate the emf of the cell at 25∘C. Write the chemical equations for the electrode reactions and represent the cell. (Given: E∘Zn2+/Zn=−0.76 volt and E∘Pb2+/Pb=−0.13 volt.

Ecell=0.76−0.13=0.63VEcell=E∘−RTnFlnQ

$E_{c e l l} = 0.76 - 0.13 = 0.63 V$
$E_{c e l l} = E^{\circ} - \frac{R T}{n F} l n Q$