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Calculate the equilibrium constant for t...

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

Text Solution

Verified by Experts

`log K_( c) = (nE_("cell")^(@))/0.0591, E_("cell")^(@) = 0.16 V, n=4`
`logK_( c) =(4 xx 0.16)/0.0591 = 10.8`
`K_(a) ="antilog" 10.8= 6.31 xx 10^(10)`
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