Writing the Equilibrium Constant Expression

Oct 13, 2025 by wbrum.org 105 views

Introduction

In chemistry, equilibrium constant expressions are used to describe the balance between reactants and products in a reversible reaction. These expressions are crucial in understanding the thermodynamic properties of a system and predicting the direction of a reaction. In this article, we will explore the concept of equilibrium constant expressions and apply it to a reversible reaction.

What is an Equilibrium Constant Expression?

An equilibrium constant expression is a mathematical representation of the equilibrium constant (K) for a reversible reaction. It is a ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their stoichiometric coefficients. The equilibrium constant expression is a fundamental concept in chemistry and is used to predict the direction of a reaction and the concentrations of the reactants and products at equilibrium.

The Given Reaction

The given reversible reaction is:

${ C(s) + O_2(g) \rightleftharpoons CO_2(g) }$

In this reaction, carbon (C) is a solid reactant, oxygen gas (O2) is a gaseous reactant, and carbon dioxide (CO2) is a gaseous product.

Writing the Equilibrium Constant Expression

To write the equilibrium constant expression for the given reaction, we need to consider the stoichiometric coefficients of the reactants and products. The stoichiometric coefficients are the numbers in front of each reactant or product in the balanced chemical equation.

In this reaction, the stoichiometric coefficients are:

C(s): 1
O2(g): 1
CO2(g): 1

The equilibrium constant expression is written as:

${ K_{\text{eq}} = \frac{[CO_2]}{[C][O_2]} }$

However, since C is a solid, its concentration is not included in the equilibrium constant expression. Therefore, the correct equilibrium constant expression for the given reaction is:

${ K_{\text{eq}} = [CO_2] }$

Why is the Concentration of C Not Included?

The concentration of a solid reactant is not included in the equilibrium constant expression because the concentration of a solid is essentially constant. This is because the volume of a solid is negligible compared to the volume of a gas or liquid, and the concentration of a solid is not affected by changes in temperature or pressure.

Conclusion

In conclusion, the equilibrium constant expression for the given reversible reaction is:

${ K_{\text{eq}} = [CO_2] }$

This expression describes the balance between the reactants and products in the reaction and is used to predict the direction of the reaction and the concentrations of the reactants and products at equilibrium.

Common Mistakes to Avoid

When writing the equilibrium constant expression, it is essential to consider the stoichiometric coefficients of the reactants and products. Additionally, the concentration of a solid reactant is not included in the equilibrium constant expression.

Example Problems

Write the equilibrium constant expression for the following reversible reaction:

${ N_2(g) + O_2(g) \rightleftharpoons 2NO(g) }$

Solution:

The stoichiometric coefficients are:

N2(g): 1
O2(g): 1
NO(g): 2

The equilibrium constant expression is:

${ K_{\text{eq}} = \frac{[NO]^2}{[N_2][O_2]} }$

Write the equilibrium constant expression for the following reversible reaction:

${ CaCO_3(s) + H^+(aq) \rightleftharpoons Ca^2+(aq) + CO_2(g) }$

Solution:

The stoichiometric coefficients are:

CaCO3(s): 1
H+(aq): 1
Ca2+(aq): 1
CO2(g): 1

The equilibrium constant expression is:

${ K_{\text{eq}} = \frac{[Ca^2+][CO_2]}{[H^+]} }$

Note that the concentration of CaCO3(s) is not included in the equilibrium constant expression.

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
Chang, R. (2010). Chemistry. McGraw-Hill.
Levine, I. N. (2012). Physical chemistry. McGraw-Hill.

Glossary

Equilibrium constant expression: A mathematical representation of the equilibrium constant (K) for a reversible reaction.
Stoichiometric coefficients: The numbers in front of each reactant or product in the balanced chemical equation.
Solid reactant: A reactant that is in the solid phase.
Gas reactant: A reactant that is in the gaseous phase.
Liquid reactant: A reactant that is in the liquid phase.
Equilibrium Constant Expressions: Frequently Asked Questions ===========================================================

Q: What is the equilibrium constant expression?

A: The equilibrium constant expression is a mathematical representation of the equilibrium constant (K) for a reversible reaction. It is a ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their stoichiometric coefficients.

Q: Why is the equilibrium constant expression important?

A: The equilibrium constant expression is important because it allows us to predict the direction of a reaction and the concentrations of the reactants and products at equilibrium. It is a fundamental concept in chemistry and is used to describe the balance between reactants and products in a reversible reaction.

Q: How do I write the equilibrium constant expression?

A: To write the equilibrium constant expression, you need to consider the stoichiometric coefficients of the reactants and products. The stoichiometric coefficients are the numbers in front of each reactant or product in the balanced chemical equation. The equilibrium constant expression is written as a ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their stoichiometric coefficients.

Q: What happens if a reactant is a solid?

A: If a reactant is a solid, its concentration is not included in the equilibrium constant expression. This is because the concentration of a solid is essentially constant and is not affected by changes in temperature or pressure.

Q: What happens if a reactant is a gas?

A: If a reactant is a gas, its concentration is included in the equilibrium constant expression. The concentration of a gas is affected by changes in temperature and pressure, so it is included in the equilibrium constant expression.

Q: Can I use the equilibrium constant expression to predict the direction of a reaction?

A: Yes, you can use the equilibrium constant expression to predict the direction of a reaction. If the equilibrium constant (K) is greater than 1, the reaction will favor the products. If the equilibrium constant (K) is less than 1, the reaction will favor the reactants.

Q: Can I use the equilibrium constant expression to predict the concentrations of the reactants and products at equilibrium?

A: Yes, you can use the equilibrium constant expression to predict the concentrations of the reactants and products at equilibrium. By rearranging the equilibrium constant expression, you can solve for the concentrations of the reactants and products.

Q: What are some common mistakes to avoid when writing the equilibrium constant expression?

A: Some common mistakes to avoid when writing the equilibrium constant expression include:

Not considering the stoichiometric coefficients of the reactants and products
Including the concentration of a solid reactant
Not including the concentration of a gas reactant
Not rearranging the equilibrium constant expression to solve for the concentrations of the reactants and products

Q: What are some examples of equilibrium constant expressions?

A: Some examples of equilibrium constant expressions include:

For the reaction: N2(g) + O2(g) ⇌ 2NO(g)
- The equilibrium constant expression is: Keq = [NO]^2 / [N2][O2]
For the reaction: CaCO3(s) + H+(aq) ⇌ Ca^2+(aq) + CO2(g)
- The equilibrium constant expression is: Keq = [Ca^2+][CO2] / [H+]

Q: Where can I find more information about equilibrium constant expressions?

A: You can find more information about equilibrium constant expressions in chemistry textbooks, online resources, and scientific articles. Some recommended resources include:

Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
Chang, R. (2010). Chemistry. McGraw-Hill.
Levine, I. N. (2012). Physical chemistry. McGraw-Hill.

Glossary

Equilibrium constant expression: A mathematical representation of the equilibrium constant (K) for a reversible reaction.
Stoichiometric coefficients: The numbers in front of each reactant or product in the balanced chemical equation.
Solid reactant: A reactant that is in the solid phase.
Gas reactant: A reactant that is in the gaseous phase.
Liquid reactant: A reactant that is in the liquid phase.