The Molar Enthalpy of Vaporization

Oct 13, 2025 by magicalceylontours.com 34 views

Introduction

In thermodynamics, the change in enthalpy ( $\Delta H$ ) is a measure of the energy change associated with a chemical or physical process. When a substance undergoes a phase transition, such as condensation, the enthalpy change can be calculated using the molar enthalpy of vaporization ( $\Delta H_v$ ). In this article, we will explore the change in enthalpy when 180 g of water vapor condenses at $100^{\circ}C$ , given that the molar enthalpy of vaporization of water is $40.67 \text{ kJ/mol}$ .

The Molar Enthalpy of Vaporization

The molar enthalpy of vaporization ( $\Delta H_v$ ) is the energy required to vaporize one mole of a substance at its boiling point. In the case of water, the molar enthalpy of vaporization is $40.67 \text{ kJ/mol}$ . This value represents the energy required to change one mole of liquid water into one mole of water vapor at $100^{\circ}C$ .

Calculating the Change in Enthalpy

To calculate the change in enthalpy when 180 g of water vapor condenses, we need to follow these steps:

Determine the number of moles of water vapor: We can calculate the number of moles of water vapor using the formula:

n = \frac{m}{M}

where $n$ is the number of moles, $m$ is the mass of water vapor (in grams), and $M$ is the molar mass of water (in grams per mole).

The molar mass of water is $18.02 \text{ g/mol}$ . Therefore, the number of moles of water vapor is:

n = \frac{180 \text{ g}}{18.02 \text{ g/mol}} = 10 \text{ mol}

Calculate the change in enthalpy: We can calculate the change in enthalpy using the formula:

\Delta H = n \times \Delta H_v

where $\Delta H$ is the change in enthalpy, $n$ is the number of moles of water vapor, and $\Delta H_v$ is the molar enthalpy of vaporization.

Substituting the values, we get:

\Delta H = 10 \text{ mol} \times 40.67 \text{ kJ/mol} = 406.7 \text{ kJ}

Rounding the Answer

The calculated value of $\Delta H$ is $406.7 \text{ kJ}$ . However, the answer choices are given in whole numbers. Therefore, we can round the answer to the nearest whole number.

Rounding $406.7 \text{ kJ}$ to the nearest whole number, we get:

\Delta H \approx 407 \text{ kJ}

Conclusion

In conclusion, the change in enthalpy when 180 g of water vapor condenses at $100^{\circ}C$ is approximately $407 \text{ kJ}$ . This value represents the energy released when the water vapor condenses into liquid water.

Answer

The correct answer is:

C. $407 \text{ kJ}$

Discussion

This problem requires a basic understanding of thermodynamics and the concept of enthalpy. The student should be able to calculate the number of moles of water vapor and then use the molar enthalpy of vaporization to calculate the change in enthalpy.

Additional Practice Problems

Calculate the change in enthalpy when 120 g of water vapor condenses at $100^{\circ}C$ .
Calculate the change in enthalpy when 240 g of water vapor condenses at $100^{\circ}C$ .
Calculate the change in enthalpy when 180 g of water vapor condenses at $80^{\circ}C$ .

References

CRC Handbook of Chemistry and Physics: This reference provides the molar enthalpy of vaporization of water as $40.67 \text{ kJ/mol}$ .
Thermodynamics: This reference provides a detailed explanation of the concept of enthalpy and its application in thermodynamics.
Q&A: Understanding the Change in Enthalpy During Condensation ===========================================================

Introduction

In our previous article, we explored the change in enthalpy when 180 g of water vapor condenses at $100^{\circ}C$ . In this article, we will answer some frequently asked questions related to this topic.

Q: What is the molar enthalpy of vaporization of water?

A: The molar enthalpy of vaporization of water is $40.67 \text{ kJ/mol}$ . This value represents the energy required to change one mole of liquid water into one mole of water vapor at $100^{\circ}C$ .

Q: How do I calculate the change in enthalpy when water vapor condenses?

A: To calculate the change in enthalpy when water vapor condenses, you need to follow these steps:

Determine the number of moles of water vapor using the formula: $n = \frac{m}{M}$ , where $n$ is the number of moles, $m$ is the mass of water vapor (in grams), and $M$ is the molar mass of water (in grams per mole).
Calculate the change in enthalpy using the formula: $\Delta H = n \times \Delta H_v$ , where $\Delta H$ is the change in enthalpy, $n$ is the number of moles of water vapor, and $\Delta H_v$ is the molar enthalpy of vaporization.

Q: What is the difference between the change in enthalpy and the molar enthalpy of vaporization?

A: The change in enthalpy ( $\Delta H$ ) is the energy change associated with a chemical or physical process, while the molar enthalpy of vaporization ( $\Delta H_v$ ) is the energy required to vaporize one mole of a substance at its boiling point.

Q: Can I use the change in enthalpy to calculate the energy released during condensation?

A: Yes, you can use the change in enthalpy to calculate the energy released during condensation. The energy released during condensation is equal to the negative of the change in enthalpy.

Q: What is the significance of the change in enthalpy during condensation?

A: The change in enthalpy during condensation is significant because it represents the energy released when water vapor condenses into liquid water. This energy can be used to perform work or to heat up the surroundings.

Q: Can I apply the concept of change in enthalpy to other phase transitions?

A: Yes, you can apply the concept of change in enthalpy to other phase transitions, such as melting, freezing, and sublimation.

Q: What are some common applications of the concept of change in enthalpy?

A: Some common applications of the concept of change in enthalpy include:

Calculating the energy released during condensation
Calculating the energy required to vaporize a substance
Understanding the thermodynamic properties of a substance
Designing heat exchangers and other thermal systems

Conclusion

In conclusion, the change in enthalpy during condensation is an important concept in thermodynamics that can be used to calculate the energy released during condensation. By understanding the concept of change in enthalpy, you can apply it to other phase transitions and design thermal systems that are efficient and effective.

Additional Resources

CRC Handbook of Chemistry and Physics: This reference provides the molar enthalpy of vaporization of water as $40.67 \text{ kJ/mol}$ .
Thermodynamics: This reference provides a detailed explanation of the concept of enthalpy and its application in thermodynamics.
Heat Transfer: This reference provides a detailed explanation of heat transfer and its application in thermal systems.