In a chemical equilibrium involving the reaction Q ⇌ S, which direction will the reaction favor if both Q and S are present in high concentrations?

• A. The reaction will favor the formation of Q.
• B. The reaction will favor the formation of S.
• C. The reaction will favor the formation of both Q and S equally.
• D. The reaction will remain at equilibrium with no net change.

Answer: (D)

Verified step by step guidance

1. Identify the concept of chemical equilibrium: In a chemical equilibrium, the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in the concentrations of reactants and products over time.
2. Understand the role of concentration in equilibrium: According to Le Chatelier's Principle, if a system at equilibrium is disturbed by changing the concentration of reactants or products, the system will adjust to counteract the disturbance and restore a new equilibrium.
3. Analyze the given scenario: Both Q and S are present in high concentrations. This implies that the system is already at equilibrium or close to it, as both reactants and products are available in significant amounts.
4. Consider the effect of high concentrations: High concentrations of both Q and S suggest that the reaction has reached a state where the forward and reverse reactions are occurring at the same rate, maintaining equilibrium.
5. Conclude the direction of the reaction: Since both Q and S are present in high concentrations and the system is at equilibrium, there will be no net change in the concentrations of Q and S, meaning the reaction will remain at equilibrium.