Question

Evaluate this statement: A low value for Keq means that both the forward and reverse reactions are occurring slowly.

Short answer

The statement is incorrect. A low value for Keq indicates that at equilibrium, the concentrations of reactants are high, and the concentrations of products are low, meaning that the forward reaction is not favored. However, Keq does not provide information about the speed of forward and reverse reactions. It only represents the relative concentrations of reactants and products at equilibrium.

Step-by-step solution

Defining Keq

The equilibrium constant, Keq, is a dimensionless quantity that indicates the relative concentrations of reactants and products when a chemical reaction reaches equilibrium. Keq is given by the ratio of the product of concentrations of products to the product of concentrations of reactants, each raised to the power of their respective stoichiometric coefficients. Mathematically, if the general reaction is given by: \(aA + bB ⇌ cC + dD\) Then, \[Keq = \frac{[C]^c[D]^d} {[A]^a[B]^b}\] Where [A], [B], [C], and [D] represent the equilibrium concentrations of the substances involved in the reaction.

Understanding equilibrium

At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. This means that the reactant concentrations no longer change, and the reaction appears to have stopped, although the forward and reverse reactions continue to occur at the same rate.

Relating Keq to reaction rates

It is essential to understand that Keq is not directly related to the reaction rates. The value of Keq depends on the concentrations of the reactants and products at equilibrium and provides no information about how fast the reaction proceeds to reach equilibrium. A low value of Keq indicates that, at equilibrium, the concentrations of the reactants are high, and the concentrations of the products are low. This means that the forward reaction is not favored, and the reaction mixture consists predominantly of reactants.

Evaluating the statement

The given statement says that "A low value for Keq means that both the forward and reverse reactions are occurring slowly." From the previous steps, it is clear that Keq provides information about the concentrations of reactants and products at equilibrium and not their rates. Thus, the given statement is incorrect. A low value for Keq does not imply that both the forward and reverse reactions are occurring slowly. It simply means that, at equilibrium, the reaction mixture consists mainly of reactants, and the forward reaction is not favored.

Key concepts

Chemical Equilibrium

When a chemical reaction reaches a state where the concentrations of reactants and products remain constant over time, it is said to be in chemical equilibrium. This does not mean that the reactions have stopped. Instead, it implies that the forward and reverse reactions occur at the same rate.
For example, consider the reversible reaction:

• \(aA + bB ⇌ cC + dD\)

Once equilibrium is achieved, the concentrations of \(A\), \(B\), \(C\), and \(D\) do not change. It is akin to a state of balance where there is no net change in the amount of reactants and products.
Remember, reaching equilibrium does not mean equal concentrations, but a stable ratio according to the equilibrium constant \(Keq\).
The concept of chemical equilibrium is fundamental in understanding many phenomena in chemistry, including reaction dynamics and catalysis.

Reaction Rates

Reaction rates refer to how quickly reactants are converted into products in a chemical reaction. The rate can vary significantly depending on several factors like temperature, pressure, concentration, and catalysts.
Understanding the reaction rates can give insight into the mechanism of the reaction. A reaction can be fast or slow regardless of the equilibrium constant \(Keq\).
Factors affecting reaction rates include:

• **Concentration**: Higher concentration tends to increase the rate.
• **Temperature**: Generally, higher temperatures increase reaction rates.
• **Catalysts**: These substances increase reaction rates without being consumed.

It's important to distinguish that \(Keq\) does not dictate how fast the equilibrium is reached; it only describes the state once equilibrium is achieved.

Reactants and Products Concentrations

In any chemical reaction at equilibrium, the concentrations of reactants and products are linked through the equilibrium constant \(Keq\). This constant provides a snapshot of the balance between products and reactants at equilibrium.
For instance, if \(Keq\) is low, it signifies that the concentration of reactants is higher compared to the concentration of products at equilibrium. This means that the reaction favors the reactants.
In the reaction example:

• \(aA + bB ⇌ cC + dD\),

The equilibrium expression is:\[Keq = \frac{[C]^c[D]^d}{[A]^a[B]^b}\]The relationship given by this expression shows that equilibrium can have different concentrations depending on the specific \(Keq\) value. It also helps predict how shifts in concentration, temperature, or pressure can alter the equilibrium position.