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Calculate the value of equilibrium const...

Calculate the value of equilibrium constant of the reaction occurring in Deniell cell at `25^(@)C`.
Given : `E_(Zn^(2+)|Zn)^(@)=-0.76V and E_(Cu^(2+)|Cu)^(@)=+0.34V`

Text Solution

Verified by Experts

Daniell cell : `Zn|Zn^(2+)||Cu^(2+)|Cu`
`{:("Anode reaction : "Zn(s)" "rarr" "Zn^(2+)(aq)+2e),("Cathode reaction : "Cu^(2+)(Aq)+2e" "rarr" "Cu(s)),(bar(" Cell reaction : "Zn(s)+Cu^(2+)(aq)" "rarr" "Zn^(2+)(aq)+Cu(s))):}`
As 2 mole of electrons are involved in the cell reaction, n = 2.`E_("cell")^(@)=E_("cathode")^(@)-E_("anode")^(@)=E_(Cu^(2+)|Cu)^(@)-E_(Zn^(2+)|Zn^(@)`
`=[0.34-(-0.76)]=1.10V`
`logK=(nFE^(@))/(2.303RT)=(2xx96500xx1.1)/(2.303xx8.314xx298)=37.2`
`therefore" "K=1.584 xx10^(37)`
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