Q. 435.0( 1 Vote )

Match Column (I)

Answer :

We know that,

∆G = ∆G° + RTln K… eq (1)


• ∆G = Gibbs free energy


• ∆G° = Standard Gibbs free energy (1atm pressure and 298k)


• T = temperature (in kelvin)


R = Gas constant


• K = Equilibrium constant


• At Equilibrium, ∆G = 0


∆G° + RTln K = 0


So, RTln K = -∆G°...eq (2)


From the eq (2) we get smaller the magnitude of -∆G°, the higher the rate constant K will be and the faster the reaction.


(i) Equilibrium - (c) ∆G = 0


Explanation: When ∆G is equal to zero and K =1, it means Solution that at Equilibrium, the products and the reactants are equally favoured.


(ii) Spontaneous reaction - (d) ∆G < 0, K >1


Explanation: when ΔG<0, then K >1 i.e. reaction will move in the forward direction and can be used to do some useful work.


(iii) Non spontaneous reaction - (a) ∆G > 0, K < 1


Explanation: when ΔG>0, then K <1 i.e. reaction will move in the backward direction and we need external energy if we want to do some useful work.


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