Standard States and Enthalpy of Formation

Oct 13, 2025 by windailys.com 20 views

Understanding Enthalpy of Formation: A Key Concept in Chemistry

Enthalpy of formation, denoted by $\Delta H_{f}$ , is a crucial concept in chemistry that helps us understand the energy changes associated with the formation of compounds from their constituent elements. In this article, we will delve into the concept of enthalpy of formation and identify the substances that have $\Delta H_{f} = 0 \text{ kJ/mol}$ by definition.

What is Enthalpy of Formation?

Enthalpy of formation is the change in enthalpy that occurs when one mole of a compound is formed from its constituent elements in their standard states. It is a measure of the energy change associated with the formation of a compound, and it is typically expressed in units of kJ/mol. The enthalpy of formation is a fundamental property of a compound, and it can be used to predict the energy changes associated with various chemical reactions.

Standard States and Enthalpy of Formation

In order to understand the concept of enthalpy of formation, it is essential to know the standard states of the elements involved. The standard state of an element is the state in which the element exists at a pressure of 1 atm and a temperature of 25°C. For example, the standard state of oxygen is $O_2(g)$ , while the standard state of iron is $Fe(s)$ .

Substances with $\Delta H_{f} = 0 \text{ kJ/mol}$

By definition, the enthalpy of formation of an element in its standard state is zero. This is because the formation of an element from its constituent atoms does not involve any energy change. Therefore, the substances that have $\Delta H_{f} = 0 \text{ kJ/mol}$ by definition are:

A. $O_2(g)$ : Oxygen is an element that exists in its standard state as a diatomic molecule. Therefore, the enthalpy of formation of $O_2(g)$ is zero.
B. $N_2(g)$ : Nitrogen is an element that exists in its standard state as a diatomic molecule. Therefore, the enthalpy of formation of $N_2(g)$ is zero.
E. $Fe(s)$ : Iron is an element that exists in its standard state as a solid. Therefore, the enthalpy of formation of $Fe(s)$ is zero.

Substances with Non-Zero Enthalpy of Formation

On the other hand, the substances that do not have $\Delta H_{f} = 0 \text{ kJ/mol}$ are:

C. $H_2O(l)$ : Water is a compound that is formed from hydrogen and oxygen. The enthalpy of formation of $H_2O(l)$ is not zero, as it requires energy to form the bonds between the hydrogen and oxygen atoms.
D. $Br_2(l)$ : Bromine is a compound that is formed from bromine atoms. The enthalpy of formation of $Br_2(l)$ is not zero, as it requires energy to form the bonds between the bromine atoms.
F. $He(g)$ : Helium is a noble gas that exists in its standard state as a monatomic gas. However, the enthalpy of formation of $He(g)$ is not zero, as it requires energy to form the bonds between the helium atoms.

Conclusion

In conclusion, the substances that have $\Delta H_{f} = 0 \text{ kJ/mol}$ by definition are $O_2(g)$ , $N_2(g)$ , and $Fe(s)$ . These substances are elements that exist in their standard states, and their enthalpy of formation is zero. On the other hand, the substances that do not have $\Delta H_{f} = 0 \text{ kJ/mol}$ are $H_2O(l)$ , $Br_2(l)$ , and $He(g)$ , which are compounds that require energy to form the bonds between their constituent atoms.

Key Takeaways

Enthalpy of formation is a measure of the energy change associated with the formation of a compound from its constituent elements.
The standard state of an element is the state in which the element exists at a pressure of 1 atm and a temperature of 25°C.
The enthalpy of formation of an element in its standard state is zero.
The substances that have $\Delta H_{f} = 0 \text{ kJ/mol}$ by definition are $O_2(g)$ , $N_2(g)$ , and $Fe(s)$ .

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Chang, R. (2010). Chemistry (10th ed.). McGraw-Hill.
Levine, I. N. (2014). Physical chemistry (7th ed.). McGraw-Hill.
Q&A: Enthalpy of Formation and Standard States

In our previous article, we discussed the concept of enthalpy of formation and identified the substances that have $\Delta H_{f} = 0 \text{ kJ/mol}$ by definition. In this article, we will answer some frequently asked questions related to enthalpy of formation and standard states.

Q: What is the difference between enthalpy of formation and enthalpy of reaction?

A: Enthalpy of formation is the change in enthalpy that occurs when one mole of a compound is formed from its constituent elements in their standard states. Enthalpy of reaction, on the other hand, is the change in enthalpy that occurs when a chemical reaction takes place. While enthalpy of formation is a measure of the energy change associated with the formation of a compound, enthalpy of reaction is a measure of the energy change associated with a specific chemical reaction.

Q: Why is it important to know the standard state of an element?

A: The standard state of an element is the state in which the element exists at a pressure of 1 atm and a temperature of 25°C. Knowing the standard state of an element is essential in calculating the enthalpy of formation of a compound. If the standard state of an element is not known, it is difficult to calculate the enthalpy of formation of a compound.

Q: Can the enthalpy of formation of a compound be negative?

A: Yes, the enthalpy of formation of a compound can be negative. This means that the formation of the compound from its constituent elements is an exothermic process, releasing energy into the surroundings.

Q: What is the relationship between enthalpy of formation and bond energy?

A: The enthalpy of formation of a compound is related to the bond energy of the compound. The bond energy is the energy required to break a bond between two atoms. The enthalpy of formation of a compound is the sum of the bond energies of the bonds formed between the constituent atoms.

Q: Can the enthalpy of formation of a compound be zero?

A: Yes, the enthalpy of formation of a compound can be zero. This means that the formation of the compound from its constituent elements does not involve any energy change.

Q: What is the significance of the enthalpy of formation of an element in its standard state?

A: The enthalpy of formation of an element in its standard state is zero. This means that the formation of an element from its constituent atoms does not involve any energy change.

Q: Can the enthalpy of formation of a compound be used to predict the energy change associated with a chemical reaction?

A: Yes, the enthalpy of formation of a compound can be used to predict the energy change associated with a chemical reaction. By knowing the enthalpy of formation of the reactants and products, it is possible to calculate the energy change associated with the reaction.

Q: What is the relationship between enthalpy of formation and entropy?

A: The enthalpy of formation of a compound is related to the entropy of the compound. The entropy is a measure of the disorder or randomness of a system. The enthalpy of formation of a compound is the sum of the enthalpies of formation of the bonds formed between the constituent atoms, and the entropy of the compound is related to the disorder or randomness of the bonds.

Q: Can the enthalpy of formation of a compound be used to predict the spontaneity of a chemical reaction?

A: Yes, the enthalpy of formation of a compound can be used to predict the spontaneity of a chemical reaction. By knowing the enthalpy of formation of the reactants and products, it is possible to calculate the energy change associated with the reaction, and determine whether the reaction is spontaneous or not.

Conclusion

In conclusion, the enthalpy of formation is a fundamental concept in chemistry that helps us understand the energy changes associated with the formation of compounds from their constituent elements. By knowing the enthalpy of formation of a compound, it is possible to predict the energy change associated with a chemical reaction, and determine whether the reaction is spontaneous or not. We hope that this Q&A article has provided a better understanding of the concept of enthalpy of formation and its significance in chemistry.

Key Takeaways

Enthalpy of formation is a measure of the energy change associated with the formation of a compound from its constituent elements.
The standard state of an element is the state in which the element exists at a pressure of 1 atm and a temperature of 25°C.
The enthalpy of formation of an element in its standard state is zero.
The enthalpy of formation of a compound can be used to predict the energy change associated with a chemical reaction.
The enthalpy of formation of a compound can be used to predict the spontaneity of a chemical reaction.

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Chang, R. (2010). Chemistry (10th ed.). McGraw-Hill.
Levine, I. N. (2014). Physical chemistry (7th ed.). McGraw-Hill.