How does the values of equilibrium constant predict the extent of reaction?

Explanation

A. For a general equation
`aA+bBhArrcC+dD`
`K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b))`
If `K_(c)` value is more, the products formed are more. So the formed reaction takes place. If `K_(c)gt1` the forward reaction takes place more and the products formed are more. If the value of `K_(c)lt1` the products formed are less. So the reaction takes place less than 50%.