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Write Nernst equation and calculate the ...

Write Nernst equation and calculate the e.m.f of the following cell at 298 K:
`Zn|Zn^(2+)(0.01M)||Fe^(2+)(0.005M)|Fe`
Given that:
`(Zn^(2+)//Zn)=-0.763V and E_(Fe^(2+)//Fe)^(@)=-0.44V" "log2=0.3010`.

Text Solution

Verified by Experts

At anode, `Zn rarr Zn^(2+) + 2e^(-)`
At cathode,
`ul(Fe^(2+) + 2e^(-) rarr Fe)`
`ul(Zn + Fe^(2+) rarr Zn^(2+)+ Fe)`
`E= E^(@)- (0.059)/(2)"log" ([Zn^(2+)])/([Fe^(2+)])`
`=0.323 -(0.059)/(2) xx 0.301`
`=0.323- 0.008879= 0.31V`
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ACCURATE PUBLICATION-ELECTRO CHEMISTRY-Numbericals Practice
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