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Why is an external emf of more than `2.2V` required for the extraction of `CI_(2)` from brine? |
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Answer» The oxidation reaction involved in the oxidation of `Cl^(-) " ions to " Cl_(2)` is : `2Cl^(-)(aq)+2H_(2)O(l) to 2OH^(-)(aq)+H_(2)(g)+ Cl_(2)(g)` The value of `DeltaG^(@)` for the reaction is `+422` kJ (standard value). The `E_("Cell")^(@)` can be calculated as , `DeltaG^(@)=- nF E_("Cell")^(@) " or " E_("Cell")^(@)=- (DeltaG^(@))/(nF)` `DeltaG^(@)=422 kJ =422000 J=422000 CV, n=2, `E_("Cell")^(@)=-((422000 CV))/((2xx96500 C))=-2.19~~-2*20 V`. Since `E_("Cell")^(@)` comes out to be `-2*20` V for the electrolytic cell involving the oxidation of `Cl^(-)` ions, an external emf of more than 2.2 V is needed. |
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