Endothermic and Exothermic Reactions

Oct 13, 2025 by recoveryshake.com 28 views

Enthalpy change is a crucial concept in chemistry that helps us understand the energy changes that occur during chemical reactions. It is a measure of the heat energy absorbed or released by a system during a reaction. In this article, we will explore the chemical equations that can be used to represent the enthalpy change for a given reaction.

What is Enthalpy Change?

Enthalpy change, denoted by the symbol ΔH, is the change in the total energy of a system. It is a measure of the energy absorbed or released by a system during a reaction. Enthalpy change can be either positive or negative, depending on whether the reaction is endothermic or exothermic.

Endothermic and Exothermic Reactions

Endothermic reactions are those that absorb energy from the surroundings, resulting in a positive enthalpy change. Examples of endothermic reactions include the melting of ice and the decomposition of ammonia.

Exothermic reactions, on the other hand, release energy to the surroundings, resulting in a negative enthalpy change. Examples of exothermic reactions include the combustion of gasoline and the reaction between sodium and water.

Representing Enthalpy Change in Chemical Equations

Chemical equations can be used to represent the enthalpy change for a given reaction. The enthalpy change is typically represented by the symbol ΔH and is usually given in units of kJ/mol.

Example 1: Enthalpy Change in the Formation of Iron(III) Oxide

The following equation represents the formation of iron(III) oxide from iron(II) oxide and oxygen:

$4 \, \text{FeO} + \text{O}_2 \rightarrow 2 \, \text{Fe}_2\text{O}_3$

To represent the enthalpy change for this reaction, we can add the enthalpy change value to the equation:

$4 \, \text{FeO} + \text{O}_2 + 560.66 \, \text{kJ} \rightarrow 2 \, \text{Fe}_2\text{O}_3$

Example 2: Enthalpy Change in the Decomposition of Ammonia

The following equation represents the decomposition of ammonia into nitrogen and hydrogen:

$2 \, \text{NH}_3 \rightarrow \text{N}_2 + 3 \, \text{H}_2$

To represent the enthalpy change for this reaction, we can add the enthalpy change value to the equation:

$2 \, \text{NH}_3 + 46.11 \, \text{kJ} \rightarrow \text{N}_2 + 3 \, \text{H}_2$

Which Chemical Equations Can Be Used to Represent Enthalpy Change?

Based on the examples above, we can conclude that the following chemical equations can be used to represent the enthalpy change for a given reaction:

$4 \, \text{FeO} + \text{O}_2 + 560.66 \, \text{kJ} \rightarrow 2 \, \text{Fe}_2\text{O}_3$
$2 \, \text{NH}_3 + 46.11 \, \text{kJ} \rightarrow \text{N}_2 + 3 \, \text{H}_2$

Conclusion

In conclusion, chemical equations can be used to represent the enthalpy change for a given reaction. The enthalpy change is typically represented by the symbol ΔH and is usually given in units of kJ/mol. By adding the enthalpy change value to the equation, we can represent the energy changes that occur during a reaction.

References

Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2006). General chemistry: Principles and modern applications. Pearson Prentice Hall.
Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.

Frequently Asked Questions

Q: What is enthalpy change?

A: Enthalpy change is a measure of the heat energy absorbed or released by a system during a reaction.

Q: What is the difference between endothermic and exothermic reactions?

A: Endothermic reactions absorb energy from the surroundings, resulting in a positive enthalpy change. Exothermic reactions release energy to the surroundings, resulting in a negative enthalpy change.

Q: How is enthalpy change represented in chemical equations?

Enthalpy change is a fundamental concept in chemistry that helps us understand the energy changes that occur during chemical reactions. In this article, we will answer some of the most frequently asked questions about enthalpy change.

Q: What is enthalpy change?

A: Enthalpy change is a measure of the heat energy absorbed or released by a system during a reaction. It is a crucial concept in chemistry that helps us understand the energy changes that occur during chemical reactions.

Q: What is the difference between endothermic and exothermic reactions?

Q: How is enthalpy change represented in chemical equations?

A: Enthalpy change is typically represented by the symbol ΔH and is usually given in units of kJ/mol. It can be added to the equation to represent the energy changes that occur during a reaction.

Q: What is the unit of enthalpy change?

A: The unit of enthalpy change is typically given in units of kJ/mol (kilojoules per mole).

Q: Can enthalpy change be positive or negative?

A: Yes, enthalpy change can be either positive or negative. A positive enthalpy change indicates an endothermic reaction, while a negative enthalpy change indicates an exothermic reaction.

Q: How is enthalpy change related to the energy of a reaction?

A: Enthalpy change is directly related to the energy of a reaction. A positive enthalpy change indicates that the reaction requires energy to proceed, while a negative enthalpy change indicates that the reaction releases energy.

Q: Can enthalpy change be used to predict the spontaneity of a reaction?

A: Yes, enthalpy change can be used to predict the spontaneity of a reaction. A negative enthalpy change indicates that the reaction is spontaneous, while a positive enthalpy change indicates that the reaction is non-spontaneous.

Q: What is the relationship between enthalpy change and entropy change?

A: Enthalpy change and entropy change are related through the equation ΔG = ΔH - TΔS, where ΔG is the Gibbs free energy change, ΔH is the enthalpy change, T is the temperature, and ΔS is the entropy change.

Q: Can enthalpy change be used to calculate the energy of a reaction?

A: Yes, enthalpy change can be used to calculate the energy of a reaction. The energy of a reaction can be calculated using the equation ΔE = ΔH, where ΔE is the energy change and ΔH is the enthalpy change.

Conclusion

In conclusion, enthalpy change is a fundamental concept in chemistry that helps us understand the energy changes that occur during chemical reactions. By understanding enthalpy change, we can predict the spontaneity of a reaction, calculate the energy of a reaction, and understand the relationship between enthalpy change and entropy change.

References

Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2006). General chemistry: Principles and modern applications. Pearson Prentice Hall.
Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.

Glossary

Enthalpy change: A measure of the heat energy absorbed or released by a system during a reaction.
Endothermic reaction: A reaction that absorbs energy from the surroundings, resulting in a positive enthalpy change.
Exothermic reaction: A reaction that releases energy to the surroundings, resulting in a negative enthalpy change.
ΔH: The symbol for enthalpy change.
kJ/mol: The unit of enthalpy change, representing kilojoules per mole.