1.

Which of the following reaction can be possible with electrochemical cell by using E_(Cl_(2)|2Cl^(-))^(@)=1.36V and E_(Br_(2)|2Br^(-))^(@)=1.09V

Answer»

`Br_(2)+2Cl^(-) to 2Br^(-)+Cl_(2)`
`2Br^(-)+Cl_(2) to Br_(2)+2Cl^(-)`
`2Cl^(-)+2Br^(-) to Cl_(2)+2Br^(-)`
`2Br^(-) +Br_(2) to 2Cl^(-)+2Br^(-)`

SOLUTION :`E_(Cl_(2)|2Cl^(-))^(THETA)=1.36V,E_(Br_(2)|2Br^(-))^(Theta)=1.09V`

Reduction : `Cl_(2)+2e^(-) to 2Cl^(-),E_(Cl_(2)|2Cl^(-))^(Theta)=1.36V`
Oxidation : `2Br^(-)+Br_(2) to 2e,E_(Br_(2)|2Br^(-))^(Theta)=1.09V`
`E_("Reaction")^(Theta)=E_(Cl_(2)|2Cl^(-))^(Theta)-E_(Br_(2)|2Br^(-))^(Theta)`
`=1.36V-1.09V`
=0.27V
So, the one with higher value of `E^(@)` value gives reduction reaction and so, in only reaction (B), in which `Cl_(2)` ACTING as OXIDIZING agent.


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