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प्रश्न
Write the cell representation and calculate equilibrium constant for the following redox reaction:
`Ni_((s))+2Ag_((aq))^+ (1M)->Ni_((aq))^(2+)(1M)+2Ag_((s)) " at "25^@ C`
`E_(ni)^+`=-0.25V and `E_(Ag)^+=0.799V`
बेरीज
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उत्तर
`Ni_((s))+2Ag_((aq))^+ (1M)->Ni_((aq))^(2+)(1M)+2Ag_((s)) " at "25^@ C`
`E_(ni)^+`=-0.25V and `E_(Ag)^+=0.799V`
Cell representation :
`Ni_((s))|Ni_((aq))^(2+)(1M)||Ag_(aq)^+(1M)|Ag(s)`
Calculation of equilibrium constant
`E_(cell)^@=0.0592/n log_10K`
`E_"cell"^@=E_"Ag"^@-E_"Ni"^@`
=0.799-(-0.25)=1.049 V
Hence `1.049=(0.0592)/2 log_10K`
`log_10K=(1.049xx2)/0.0592=35.44`
`K=antilog(35.44)`
`=2.754xx10^35`
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