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Chapter 10: Problem 3

Define the terms equilibrium constant and equilibrium constant expression.

Short Answer

Expert verified
The equilibrium constant \( K \) is a numeric value reflecting the ratio of product to reactant concentrations at equilibrium. The equilibrium constant expression is the equation defining \( K \) based on reaction stoichiometry.

Step by step solution

01

Understanding Equilibrium

In a chemical reaction, equilibrium is the state at which the rate of the forward reaction equals the rate of the reverse reaction. At this point, the concentrations of products and reactants remain constant over time.
02

Defining Equilibrium Constant

The equilibrium constant, denoted as \( K \), is a numerical value that describes the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction. Its value provides insights into the position of equilibrium; a large \( K \) implies more products at equilibrium, and a small \( K \) implies more reactants.
03

Constructing Equilibrium Constant Expression

The equilibrium constant expression is a mathematical representation of the equilibrium constant \( K \). For a reversible reaction of the form \( aA + bB \rightleftharpoons cC + dD \), the expression is given by \( K = \frac{[C]^c [D]^d}{[A]^a [B]^b} \), where \([A]\), \([B]\), \([C]\), and \([D]\) are the equilibrium concentrations of the respective species and \( a, b, c, \) and \( d \) are their stoichiometric coefficients.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Equilibrium
Chemical equilibrium occurs in a closed system when the rate of the forward reaction equals the rate of the reverse reaction. In such a state, the concentrations of both reactants and products remain constant over time. However, it's important to note that this does not necessarily mean they are equal.
In the world of chemistry, reaching equilibrium means that the reaction is balanced, and no further visible changes occur, even though microscopic changes continue as particles keep reacting back and forth.
  • This balance helps us understand how and when reactions stabilize.
  • Equilibrium is dynamic, meaning the molecules continue moving and reacting even at equilibrium.
  • The equilibrium state is influenced by temperature, pressure, and concentration.
Getting comfortable with the concept of chemical equilibrium is crucial for predicting how different conditions impact a chemical reaction.
Reaction Rates
Reaction rates refer to the speed at which reactants are converted into products. They are critical to understanding chemical equilibrium because equilibrium is achieved when the forward and reverse reaction rates are equal.
Several factors affect reaction rates, including concentration, temperature, and the presence of catalysts:
  • Higher concentrations typically increase the rate of reaction because more molecules mean more collisions.
  • Increased temperature generally speeds up reactions as molecules move faster and collide more often.
  • Catalysts speed up reactions by lowering the activation energy needed for a reaction to occur.
Studying reaction rates helps chemists control and optimize reactions, which is essential in industrial applications and labs.
Equilibrium Constant Expression
The equilibrium constant expression is a mathematical way to understand the concentration ratio of products to reactants in a reversible chemical reaction at equilibrium. This expression is denoted as \( K \).
For a generic reaction \( aA + bB \rightleftharpoons cC + dD \), the equilibrium constant expression would be \( K = \frac{[C]^c [D]^d}{[A]^a [B]^b} \). Here is how it operates:
  • The square brackets \([ ]\) represent the equilibrium concentrations of each species.
  • The letters \(a, b, c,\) and \(d\) are the stoichiometric coefficients from the balanced reaction equation.
  • Large \( K \) indicates a high concentration of products, while small \( K \) indicates a high concentration of reactants.
Understanding these expressions assists chemists in determining the extent to which a reaction proceeds, which is invaluable for predicting yields in reactions and manufacturing processes.

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Most popular questions from this chapter

Write equilibrium constant expressions for the following reactions. (a) \(\mathrm{O}_{2}(g)+2 \mathrm{~F}_{2}(g) \rightleftarrows 2 \mathrm{OF}_{2}(g)\) (b) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftarrows 2 \mathrm{SO}_{3}(g)\) (c) \(2 \mathrm{SO}_{3}(g)+2 \mathrm{Cl}_{2}(g) \rightleftarrows 2 \mathrm{SO}_{2} \mathrm{Cl}_{2}(g)+\mathrm{O}_{2}(g)\)

The equilibrium constant for the following reaction is $$\begin{array}{l} 1.6 \times 10^{-5} \text {at } 35^{\circ} \mathrm{C} \\ \qquad 2 \mathrm{NOCl}(g) \rightleftarrows 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \end{array}$$ If \(1.0 \mathrm{~mol}\) of \(\mathrm{NOCl}\) is placed into an empty 1.0-L flask, what will be the equilibrium concentrations of all species? State all assumptions and show all work. Provide a justification for any assumptions.

Describe the difference between reactions that go to completion and reactions that come to equilibrium.

Write equilibrium constant expressions for the following reactions. (a) \(2 \mathrm{NO}(g)+2 \mathrm{H}_{2}(g) \rightleftarrows \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\) (b) \(2 \mathrm{NOCl}(g) \rightleftarrows 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g)\) (c) \(2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \rightleftarrows 2 \mathrm{NO}_{2}(g)\)

Write the equilibrium constant expression for the dissolving of strontium fluoride in water. $$\mathrm{SrF}_{2}(s) \rightleftarrows \mathrm{Sr}^{2+}(a q)+2 \mathrm{~F}^{-}(a q)$$ (a) When \(\mathrm{SrF}_{2}(s)\) is placed in water, the compound dissolves to produce equilibrium \(\mathrm{Sr}^{2+}\) concentration of \(5.8 \times 10^{-4} \mathrm{~mol} / \mathrm{L} .\) What is \(K_{\mathrm{sp}}\) for the reaction? (b) If \(50.00 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}\) is mixed with \(50.00 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{NaF}\), will a precipitate form? Explain your answer.
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