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A reaction with ΔG <0 always has an equilibrium constant value graeter than one.why?
According to the equation
-ΔG/RT = log K
Then if the ΔG is negative then -ΔG/RT is positive as T and R r always . In that case K will have a real positive value greater than 1. Otherwise it will have the value less than 1 when ΔG is negative .
Because a reaction with ΔG<0 is spontaneous thus eq. constant must be greater than 1 so that the reaction moves forward.It can also be analysed using formula
ΔG=2.303RTlogK
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