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The standard potential of the following ...

The standard potential of the following cell is 0.23 V at `15^(@)C` and `0.21V` at `35^(@)C`.`Pt|H_(2) |HCl(aq) |Agcl (s)|g(s)`
(i) write the cell reaction .
(ii) Calculate `DeltaH^(@)` and `DeltaS^(@)` for the cell reaction by assuming that these quantities remain unchanged in the range `15^(@)C` to `35^(@)C`.
(iii) calculate the solubility of `AgCl` in water at `25^(@)C`.
Give , the standard reduction potential of the `(Ag^(+)(aq) //Ag(s)` is 0.80 V at `25^(@) C`.

Text Solution

Verified by Experts

(i) `1/2 H_(2)(g)+AgCI(s) H^(+)(aq)+Ag(s)+CI^(-)(aq)`
(ii) `Delta^(@)=-96.5 JK^(-1) mol^(-1) DeltaH^(@)=-499987 J^(-)mol^(-1)`
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Knowledge Check

  • Calculate the standard potential of the cell ,If the standard electrode potentials of Zn^(2+)//Zn and Ag^(+) //Ag are -0.763 V and + 0.799 V respectively .

    A
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    B
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    C
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