Question

When a chemical reaction is at equilibrium, which of the following statements is always TRUE?

Answer 1

Answer: The correct answer is Option D.

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric coefficients. It is represented by $K_{eq}$

For a general chemical reaction:

$aA+bB\rightarrow cC+dD$

The $K_{eq}$ is written as:

$K_{eq}=\frac{[C]^c[D]^d}{[A]^a[B]^b}$

There are 3 conditions:

• When $K_{eq}>1$; the reaction is product favored.
• When $K_{eq}$; the reaction is reactant favored.
• When $K_{eq}=1$; the reaction is in equilibrium.

At equilibrium, the  ratio of concentration of reactants to the concentration of products is equal to 1.

At equilibrium, the rate of forward reaction is equal to rate of backward reaction.

Hence, the correct answer is Option D.