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Chapter 5: Problem 1

How can you determine whether a reaction is at chemical equilibrium?

Short Answer

Expert verified
Question: Determine whether the following reaction is at equilibrium given the initial concentrations and equilibrium constant: A (aq) + B (aq) ↔ C (aq) + D (aq), K=4.00; [A]_0 = 2.0 M, [B]_0 = 1.5 M, [C]_0 = 3.0 M, [D]_0 = 1.0 M.

Step by step solution

01

Identify the balanced chemical equation

Write down the balanced chemical equation for the reaction being considered, including the coefficients and states of the compounds involved. It's crucial to have a balanced equation so that the equilibrium constant can be correctly calculated and the reaction quotient can be determined.
02

Identify the equilibrium constant expression (K)

For a general equation of the form aA + bB ↔ cC + dD, the equilibrium constant expression will be: K = ([C]^c * [D]^d) / ([A]^a * [B]^b) Where [A], [B], [C], and [D] represent the molar concentrations of the reactants and products at equilibrium, and a, b, c, and d are the coefficients from the balanced chemical equation.
03

Calculate the reaction quotient (Q)

Using the same expression as for K but with the initial molar concentrations of the reactants and products, calculate the reaction quotient: Q = ([C_0]^c * [D_0]^d) / ([A_0]^a * [B_0]^b) Where [A_0], [B_0], [C_0], and [D_0] represent the initial molar concentrations before reaching equilibrium.
04

Compare Q and K

Determine whether the reaction is at equilibrium by comparing the values of Q and K: - If Q = K, the reaction is at equilibrium. - If Q < K, the forward reaction will proceed, as there are not enough products, and the reaction will shift towards the products to achieve equilibrium. - If Q > K, the reverse reaction will proceed, as there are too many products, and the reaction will shift towards the reactants to achieve equilibrium. By following these steps, you can determine whether a reaction is at chemical equilibrium or not, and predict the direction in which the reaction will shift to achieve equilibrium if necessary.

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Most popular questions from this chapter

What is the difference between \(K_{c} K_{p}\), and \(K_{x}\) ? For a gas-phase reaction, what is the relation between them?

Does the catalyst concentration affect the reaction rate?

For a reaction taking place at constant \(p\) and \(\mathrm{T}\), why can we say that the \(\Delta \mathrm{G}^{0}\) remains constant, but we cannot say the same for \(\Delta G\) ?

How would you define the reaction rate? Which factors can affect it?

Find the relation between \(K_{p}\) and \(K_{c}\) for the following gas-phase reaction: \(a \mathrm{~A}+b \mathrm{~B} \rightleftarrows c \mathrm{C}+d \mathrm{D}\)
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