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Calculate the reduction potential of the...

Calculate the reduction potential of the following half - cells at `25^(@)C`, (2) `PT|Cl_(2)("5 atm")|HCl("0.15 M")`
Given : `E_((1)/(2)Cl_(2)|Cl^(-))^(@)=+1.36V`

Text Solution

Verified by Experts

Reduction reaction occurring in the half - cell is :
`Cl_(2)(g)+2e rarr 2Cl^(-)(aq)`
The Nernst equation for the half - cell reaction is
`E_("Red")=E_("Red")^(@)-(0.059)/(2)log.([Cl^(-)]^(2))/(p_(Cl_(2)))`
Putting : `(Cl_(2))="5 atm, "[Cl^(-)]=0.15(M)`
and `E_("Red")^(@)=1.36V` into this equation gives
`therefore" "E_("Red")=1.36-(0.059)/(2)log.((0.15)^(2))/(5)=1.429V`
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