"All chemical reaction are reversible"-Is the statement true? Given reason for your answer.

Explanation

The statement is true. Let under definite conditions, the given reaction exists in equilibrium: `A+B hArr C+D`
Equilibrium constant of the reaction, `K_(c)=([C]xx[D])/([A]xx[B])`
(where, [A],[B],[C] and [D] are the molar concentrations of A, B, C and D at equilibrium respectively). if the reaction is irreversible, then the reactants will be exhausted and values of each of [A] and [B] will become zero (0). naturally the value of `K_(c)` will be infinity `(oo)`. now we know that `DeltaG^(0)=-RTlnK_(c)`. if `K_(c)=oo`, then `DeltaG^(@)=oo`. However `DeltaG^(@)` which represents the difference in standard free energy between the products and the reactants has a definite vlaue. its value can never be completely exhausted. hence, in any chemical reaction, both the forward and backward reactions go on simultaneously i.e., all chemical reactions are reversible.