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The e.m.f of the follwing cell at 198k ...

The e.m.f of the follwing cell at 198k is 0.1745V,
`Fe(s)//Fe^(2+)(0.1M)//H^(+)(xM)//H_(2)(g)(1bar)//Pt(s)`
Calculate the `H^(+)` ions concentration of the solution at the electrode where hydrogen is being produced .
(b) Aqueous solution of copper sulphate and silver nitrate are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be asme or different ? explain your answer.

Text Solution

Verified by Experts

The overall reaction can be represented as under
`Fe+2H^(+)rightarrowH_(2)+Fe^(2+)`
Nerst equation for the reaction may be written as :
`E_("cell")=E_("cell")- (2.303RT)/(nF)log (Fe^(2+))/([H^(+)]^(2))`
Substituting the vlaues we have
`0.1745 = 0.44- (0.05591)/(2)log""([0.1])/([H^(+)]^(2))`
log `[H^(+)]=-5`
`[H^(+)]=10^(-5)`
(b) THe mass of copper and silver depostited at the cathode will be different . The amount of different substances deposited by the same quantity of electricity passing through the electrolytic solution are directly proportional to their chemical eqyivalent. Thus , copper and silver will be deposited in the ratio of 31.75:108
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Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different ? Explain your answer.

Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same of different? Explain your answer.

Knowledge Check

  • An electrolytic cell contains aqueous solution of silver sulphate and has platinum electrons. A current is passed until 1.6 g of oxygen has been liberated at the anode. The amount of silver deposited at the cathode would be

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    B
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    B
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    C
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    D
    21.58 g

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