Question

Calculate the equilibrium constant for the cell reaction :
`4Br^(-)+O_(2)+4H^(+)rarr2Br_(2)+2H_(2)O."Given "E_(cell)^(@)=0.16 V`

Answer 1

We get that, `log K_(c)=(nE_(cell)^(@))/(0.0591)`
`E_(cell)^(@)`=0.16 V,n=4
`:. " "logK_(c)=((4)xx(0.16 V))/((0.0591 V))=10.83, K_(c)="Antilog "10.83=6.76xx10^(10)`