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1900's Physics and Wave

Electrochemic...

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Electrochemical equivalent of Ag in the reaction Ag+ + e– → Ag is

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What is the electrochemical equivalent of Ag (in gram/coulomb)? (Ag = 108; F = Faraday)

Q. The two half-cell reactions of an electrochemical cell is given as

{A g}^{+} + e^{-} ⟶ A g; E_{{A g}^{+} | A g}^{o} = - 0.3995 V

{F e}^{2 +} ⟶ {F e}^{3 +} + e^{-}; E_{{F e}^{3 +} | {F e}^{2 +}}^{o} = - 0.7120 V

The value of cell EMF will be:

Q. In simple electrochemical cell, which is in its standard state, the
half cell reactions with their appropriate reduction potential are?

P b^{2 +} + 2 e \to P b

(E^{o} = - 0.13 v)

A g^{+} + e \to A g

(E^{o} = + 0.80 v)

Q. Write the reaction of the electrochemical cell formed with the help of

E_{N i^{2 +} | N i}^{0} = - 0.23 V

E_{A g^{+} | A g}^{0} = 0.83

and give symbolic representation.

Q. Consider an electrochemical cell in which the following reaction occurs :

F e^{2 +} (a q) + A g^{+} (a q) \to A g (s) + F e^{3 +} (a q)

Then how many of following changes will decrease the cell voltage:

(i) Decrease the

[A g^{+}]

(ii) Increase in

[F e^{3 +}]

(III) Increase the amount of

A g

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