A reaction withΔG<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