Calculate the equilibrium constant for the reaction at 298K. `4Br^(-)+O_(2)+4H^(+)to2Br_(2)+2H_(2)O.` Given that `E_(cell)^(@)=0

Correct Answer - `6.747xx10^(10)`
`E_(cell)^(@)=(0.0591)/(n)"log "K_(c),0.16=(0.0591)/(4)" log "K_(c)` or `log" "K_(c)=10.8291` or `K_(c)=6.747xx10^(10)`

Calculate the equilibrium constant for the reaction at 298K. `4Br^(-)+O_(2)+4H^(+)to2Br_(2)+2H_(2)O.` Given that `E_(cell)^(@)=0.16V`.

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