(a) If Q_c < K_c, in which direction will a reaction proceed in order to reach equilibrium?

Verified step by step guidance

1. Identify the given terms: Q_c is the reaction quotient, and K_c is the equilibrium constant.
2. Understand the relationship: If Q_c < K_c, it means the concentration of products is less than what is required at equilibrium.
3. Determine the direction: The reaction will proceed in the forward direction to produce more products and reach equilibrium.
4. Visualize the process: As the reaction moves forward, the concentration of reactants will decrease, and the concentration of products will increase.
5. Conclude the reasoning: The reaction continues in the forward direction until Q_c equals K_c, achieving equilibrium.

Key Concepts

Reaction Quotient (Q_c)

The reaction quotient, Q_c, is a measure of the relative concentrations of products and reactants at any point in a reaction. It is calculated using the same expression as the equilibrium constant (K_c), but with the current concentrations instead of equilibrium concentrations. Q_c helps determine the direction in which a reaction will shift to reach equilibrium.

Equilibrium Constant (K_c)

The equilibrium constant, K_c, is a value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is a fixed value for a particular reaction under specified conditions. Comparing Q_c to K_c allows us to predict the direction of the reaction's shift towards equilibrium.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, the system will adjust to counteract the disturbance and restore a new equilibrium. In the context of Q_c and K_c, if Q_c is less than K_c, the reaction will shift to the right, favoring the formation of products to achieve equilibrium.