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Gibb's Energy and Nernst Equation

The EMF of a ...

Question

The EMF of a concentration cell consisting of two zinc electrodes, on dipping into M/4 solution of $Z n S O_{4}$ and the other M/16 solution of the same salt at $25^{\circ} C$ is:

0.0125 V

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0.0250 V

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0.0178 V

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0.0356 V

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Solution

The correct option is C $0.0178 V$
For concentration cell, $E^{⊖}$ = 0
E = $- \frac{0.059}{2} l o g \frac{(Z n^{2 +})_{a}}{(Z n^{2 +})_{c}}$
= $- \frac{0.059}{2} l o g \frac{M / 16}{M / 4}$
= $- \frac{0.059}{2} l o g (\frac{1}{4})$
E = $0.0178 V$

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Similar questions

The emf of a concentration cell consisting of two zinc electrode, one dipping into M/4 solution of zinc sulphate and the other into M/16 solution of the same salt at 25 $^{0}$ C :

Q. What is the potential of a half cell consisting of zinc electrode in 0.01 M

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Q. What is the single electrode potential of a half-cell for zinc electrode dipping in

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Q. A zinc rod is dipped in

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[E_{Z n^{+ +} / Z n}^{0} = - 0.76 e V]

Q. A cell contains two hydrogen electrodes. The negative electrode is in contact with a solution of

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The EMF of a concentration cell consisting of two zinc electrodes, on dipping into M/4 solution of ZnSO4 and the other M/16 solution of the same salt at 25∘C is:

The correct option is C 0.0178VFor concentration cell, E⊖ = 0E = −0.0592log(Zn2+)a(Zn2+)c= −0.0592logM/16M/4= −0.0592log(14)E =0.0178V

The EMF of a concentration cell consisting of two zinc electrodes, on dipping into M/4 solution of $Z n S O_{4}$ and the other M/16 solution of the same salt at $25^{\circ} C$ is:

The correct option is C $0.0178 V$
For concentration cell, $E^{⊖}$ = 0
E = $- \frac{0.059}{2} l o g \frac{(Z n^{2 +})_{a}}{(Z n^{2 +})_{c}}$
= $- \frac{0.059}{2} l o g \frac{M / 16}{M / 4}$
= $- \frac{0.059}{2} l o g (\frac{1}{4})$
E = $0.0178 V$