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Which of the following statements is FALSE?

(A) When K >> 1, the forward reaction is favored and essentially goes to completion.
(B) When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent.
(C) When K ≈ 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium.
(D) K >> 1 implies that the reaction is very fast at producing products.
(E) None of the above.

Respuesta :

andreafernandez

Answer:

D

Explanation:

D. K >> 1 implies that the reaction is very fast at producing products.

jufsanabriasa

Answer:

(D) K >> 1 implies that the reaction is very fast at producing products.

Explanation:

For a reaction:

nA + xB ⇄ bC + aD

The thermodynamic equilibrium constant (k) is:

k = [tex]\frac{[C]^b[D]^a]}{[A]^n[B]^x}[/tex] (1)

(A) When K >> 1, the forward reaction is favored and essentially goes to completion.  TRUE. By (1), a k>> 1 means that you have more products than reactants

(B) When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent.  TRUE. By (1), a k<< 1 means that you have more reactants than products.

(C) When K ≈ 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium.  TRUE. By (1), a k ≈ 1 means that you have the same concentration of products andreactants

(D) K >> 1 implies that the reaction is very fast at producing products.  FALSE. k is a thermodynamic parameter. To evaluate the rate of a reaction you need to study the kinetics of this one.

I hope it helps!

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