Which of the following statements is correct for a reaction that has K << 1? Ans

Question

Which of the following statements is correct for a reaction that has K
<< 1? Answer The forward reaction is faster than the reverse reaction. The reverse reaction is faster than the forward reaction. The equilibrium favors the products. The equilibrium favors the reactants. None of these statements is correct.

??? Which of the following statements is correct for a reaction that has K
<< 1? Answer The forward reaction is faster than the reverse reaction. The reverse reaction is faster than the forward reaction. The equilibrium favors the products. The equilibrium favors the reactants. None of these statements is correct.

??? Which of the following statements is correct for a reaction that has K
<< 1? Which of the following statements is correct for a reaction that has K
<< 1? The forward reaction is faster than the reverse reaction. The reverse reaction is faster than the forward reaction. The equilibrium favors the products. The equilibrium favors the reactants. None of these statements is correct.

??? The forward reaction is faster than the reverse reaction. The reverse reaction is faster than the forward reaction. The equilibrium favors the products. The equilibrium favors the reactants. None of these statements is correct.

???

Explanation / Answer

A large K (equilibrium constant) means that at equilibrium, the concentrations of the products will generally be greater than the concentrations of the reactants. Small K means just the opposite.

K is also related to the standard free energy change (Delta Go). A large K means that delta Go is more negative, and that under standard conditions, the reaction is exergonic and spontaneous. A small K means the reaction is endergonic and not spontaneous.

answer B

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