Question

. List three characteristics a reaction mixture must have if it is to attain a state of chemical equilibriu

Short answer

A reaction mixture must have the following three characteristics to attain a state of chemical equilibrium: (a) the rate of the forward reaction is equal to the rate of the reverse reaction, (b) the concentrations of the reactants and products remain constant over time, and (c) the equilibrium can be approached from either direction. The expression for the equilibrium constant (K) for a general reaction \(aA + bB \rightleftharpoons cC + dD\) is given by \(K = \frac{[C]^c [D]^d}{[A]^a [B]^b}\).

Step-by-step solution

1. Three characteristics of chemical equilibrium

a. The rate of the forward reaction is equal to the rate of the reverse reaction. b. The concentrations of the reactants and products remain constant over time. c. The equilibrium can be approached from either direction (i.e., from excess reactants or excess products).

2. Write the general reaction

Given the general reaction, \(aA + bB \rightleftharpoons cC + dD\) Here, a, b, c, and d are the stoichiometric coefficients of the reactants A, B, and the products C and D, respectively.

3. Write the expressions for the forward and reverse reaction rates

The rate laws for the forward reaction (Rf) and reverse reaction (Rr) can be expressed as follows: \(Rf = k_f[A]^a[B]^b\) and \(Rr = k_r[C]^c[D]^d\) Here, \(k_f\) and \(k_r\) are the rate constants for the forward and reverse reactions, respectively.

4. Equate the forward and reverse reaction rates

At chemical equilibrium, the forward and reverse reaction rates are equal: \(k_f[A]^a[B]^b = k_r[C]^c[D]^d\)

5. Derive the expression for the equilibrium constant, K

The equilibrium constant (K) can be defined as the ratio of the rate constants for the forward and reverse reactions: \(K = \frac{k_f}{k_r}\) Now, substitute the expressions for the forward and reverse reaction rates from step 4 into the K equation: \(K = \frac{k_f[A]^a[B]^b}{k_r[C]^c[D]^d}\) This simplifies to: \(K = \frac{[C]^c [D]^d}{[A]^a [B]^b}\) The expression for the equilibrium constant (K) is derived as follows: \(K = \frac{[C]^c [D]^d}{[A]^a[B]^b}\)

Key concepts

Rate of Reaction

In chemical reactions, the rate of reaction is a measure of how quickly reactants are converted into products. This rate can vary significantly from one reaction to another. The speed of any reaction is determined by factors such as temperature, concentration of reactants, and the presence of catalysts.
The rate of reaction is crucial in reaching chemical equilibrium. At equilibrium, the rates of the forward and reverse reactions are equal. This balance means that the amount of reactants turning into products is exactly matched by the products reverting to reactants.
A basic understanding of rate laws helps to explore this further. For a general reaction represented by \(aA + bB \rightleftharpoons cC + dD\), the rates of forward \(R_f\) and reverse \(R_r\) reactions can be expressed as:

• \(R_f = k_f[A]^a[B]^b\)
• \(R_r = k_r[C]^c[D]^d\)

Here, \(k_f\) and \(k_r\) are the constants that indicate how fast each reaction progresses under certain conditions.

Equilibrium Constant

The equilibrium constant \(K\) is a key concept in understanding chemical equilibrium. Represented as \(K\), it reflects the ratio of concentrations of products to reactants at equilibrium. A chemical system at equilibrium has its equilibrium constant formulated from the balanced chemical equation: \(K = \frac{[C]^c[D]^d}{[A]^a[B]^b}\).
This equation shows that \(K\) is a measure of the relative concentrations of reactants and products when the rate of forward reaction equals the rate of reverse reaction. In essence, it provides insight into the position of equilibrium.
If \(K\) is large, it implies higher concentrations of products. A smaller \(K\) suggests that reactants are favored. The equilibrium constant, thus, helps predict the extent to which a reaction will occur.

Reactant and Product Concentrations

In the context of chemical equilibrium, reactant and product concentrations remain constant when the system reaches equilibrium. This constancy does not mean the reaction has stopped but that the reactants and products are converted back and forth at equal rates.
The concentrations can be calculated once \(K\) is known, and they define the state of equilibrium for a particular reaction at a given temperature.
What's fascinating is that equilibrium can be achieved regardless of starting concentrations. Whether you start with more reactants or more products, the system will adjust to maintain the same equilibrium constant \(K\). Therefore, it is essential to understand how initial concentrations can lead to a dynamic and balanced chemical system.