Question

question 7 (1 point)
if $q_{eq} > k_{eq}$, then ______.

a) the ratio of products to reactants is less than $k_{eq}$

b) the ratio of products to reactants is greater than $k_{eq}$

c) the reaction shifts toward product formation

d) more reactants must be consumed to reach equilibrium

e) the system is at equilibrium

Explanation:

To solve this, we recall the concepts of reaction quotient (\(Q_{eq}\)) and equilibrium constant (\(K_{eq}\)). The reaction quotient \(Q_{eq}\) has the same formula as \(K_{eq}\) (ratio of products to reactants, each raised to their stoichiometric coefficients), but \(Q_{eq}\) is at any point, while \(K_{eq}\) is at equilibrium.

• Option a: If \(Q_{eq}>K_{eq}\), the ratio of products to reactants (which is \(Q_{eq}\)) is greater than \(K_{eq}\), so a is wrong.
• Option b: By definition, \(Q_{eq}\) is the ratio of products to reactants (at a given time). So if \(Q_{eq}>K_{eq}\), this ratio is greater than \(K_{eq}\). This matches.
• Option c: When \(Q_{eq}>K_{eq}\), the reaction shifts to the left (toward reactants) to reduce the amount of products and increase reactants, so c is wrong.
• Option d: To reach equilibrium, we need to form more reactants (so reactants are produced, not consumed), so d is wrong.
• Option e: The system is at equilibrium only when \(Q_{eq} = K_{eq}\), so e is wrong.

Answer:

b) the ratio of products to reactants is greater than \(K_{eq}\)