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Electrochemistry

Short Answer Type

1. How would you determine the standard electrode potential of the system Mg²⁺/Mg?

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2. Can you store copper sulphate solutions in a Zinc pot?

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3. Consult the table of standard electrode potentials and suggest three substance that can oxidize ferrous ions under suitable conditions.

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4. Calculate the potential of hydrogen electrode in contact with a solution whose pH is 10.

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Long Answer Type

5. Calculate the emf of the cell in which the following reaction takes place:
Ni(s) + 2Ag⁺ (0.002 M)

\to

Ni²⁺ (0.160 M) + 2Ag(s)
Given that

{E^{o}}_{Cell} = 1.05 V

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6. The cell in which the following reaction occurs:
2Fe³⁺ (aq) + 2I^–(aq)

\to

2Fe²⁺ (aq) + I₂(s) has E⁰_cell = 0.236 V at 298 K. Calculate the standerd Gibbs energy and the equilibrium constance of the cell reaction.

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Short Answer Type

7. Why does the conductivity of a solution decrease with dilution?

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8. Suggest a way to determine the Λ°_m value of water.

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Long Answer Type

9. The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

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Short Answer Type

10. If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

Answer:

Current, I = 0.5 A

Time, t = 2 hours

Convert in sec we get

Time, t = 2 × 60 × 60 s

= 7200 s

Use formula

Charge Q = It

Plug the values we get

= 0.5 A × 7200 s

= 3600 Coulombs

Number of electrons = total charge / charge on 1 electrons

= 3600/(1.6 ×10 ¹⁹)

=2.25 × 10²² electrons

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