Answered: H,O() = H,0(g) AH = 41 kJ

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Question

How can the pressure of water vapor be increased in the following equilibrium?

$### Phase Transition of Water In this example, we are examining the phase transition of water from liquid to gas: \[ \text{H}_2\text{O (l)} \rightleftharpoons \text{H}_2\text{O (g)} \] This equation represents the equilibrium between liquid water (H₂O (l)) and water vapor (H₂O (g)). The double-headed arrow indicates that the process can proceed in both forward and reverse directions, meaning water can evaporate to form vapor, or vapor can condense to form liquid water. ### Enthalpy Change (ΔH) The enthalpy change ($\Delta H$) for this phase transition is provided as: \[ \Delta H = 41 \text{kJ} \] This value indicates the amount of energy required to convert one mole of liquid water into one mole of water vapor under constant pressure. Specifically, $41 \text{kJ}$ is the amount of heat energy absorbed by the system from the surroundings during the phase transition from liquid to gas (endothermic process). Understanding the enthalpy change is crucial for various applications, including chemical engineering, environmental science, and physical chemistry, where accurate energy estimations are essential for process design and analysis.$

Transcribed Image Text:### Phase Transition of Water In this example, we are examining the phase transition of water from liquid to gas: \[ \text{H}_2\text{O (l)} \rightleftharpoons \text{H}_2\text{O (g)} \] This equation represents the equilibrium between liquid water (H₂O (l)) and water vapor (H₂O (g)). The double-headed arrow indicates that the process can proceed in both forward and reverse directions, meaning water can evaporate to form vapor, or vapor can condense to form liquid water. ### Enthalpy Change (ΔH) The enthalpy change ($\Delta H$) for this phase transition is provided as: \[ \Delta H = 41 \text{kJ} \] This value indicates the amount of energy required to convert one mole of liquid water into one mole of water vapor under constant pressure. Specifically, $41 \text{kJ}$ is the amount of heat energy absorbed by the system from the surroundings during the phase transition from liquid to gas (endothermic process). Understanding the enthalpy change is crucial for various applications, including chemical engineering, environmental science, and physical chemistry, where accurate energy estimations are essential for process design and analysis.

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions