Question

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.

Answer 1

D

Step-by-step explanation:

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

Answer 2

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

Step-by-step explanation:

For a reaction:

nA + xB ⇄ bC + aD

The thermodynamic equilibrium constant (k) is:

k =
`([C]^b[D]^a])/([A]^n[B]^x)` (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!