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2) While water's boiling point at 1 atm is 100 °C, if you heat water quickly, you can "superheat" it past its boiling point. Superheated water is a kinetically metastable state and will rapidly boil if disturbed. a. Consider 13 mol of water (approximately 1 cup) that have been superheated to 110 °C. What is the enthalpy change for converting this superheated liquid into water vapor at 110 °C? To calculate this, you'll need to look up the heat capacity of water, the heat capacity of water vapor, and the enthalpy of vaporization of water. You can assume each of these quantities is constant over the range 100-110 °C. b. You should find your answer differs from that for vaporizing the same amount of water at 100 °C, water's normal boiling point. Can you provide a chemical explanation as to why these two quantities should differ?

2) While water's boiling point at 1 atm is 100 °C, if you heat water quickly, you can "superheat" it past its boiling point. Superheated water is a kinetically metastable state and will rapidly boil if disturbed. a. Consider 13 mol of water (approximately 1 cup) that have been superheated to 110 °C. What is the enthalpy change for converting this superheated liquid into water vapor at 110 °C? To calculate this, you'll need to look up the heat capacity of water, the heat capacity of water vapor, and the enthalpy of vaporization of water. You can assume each of these quantities is constant over the range 100-110 °C. b. You should find your answer differs from that for vaporizing the same amount of water at 100 °C, water's normal boiling point. Can you provide a chemical explanation as to why these two quantities should differ?

Chemistry
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...
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2) While water's boiling point at 1 atm is 100 °C, if you heat water quickly, you can "superheat" it past its boiling point. Superheated water is a kinetically metastable state and will rapidly boil if disturbed. a. Consider 13 mol of water (approximately 1 cup) that have been superheated to 110 °C. What is the enthalpy change for converting this superheated liquid into water vapor at 110 °C? To calculate this, you'll need to look up the heat capacity of water, the heat capacity of water vapor, and the enthalpy of vaporization of water. You can assume each of these quantities is constant over the range 100 110 °C. b. You should find your answer differs from that for vaporizing the same amount of water at 100 °C, water's normal boiling point. Can you provide a chemical explanation as to why these two quantities should differ? 3) What is the probability that 100 ideal gas particles will spontaneously contract their volume by 0.01%? What about 1000 ideal gas particles? How many molecules do you need to consider before the probability of contraction becomes less than 1%? Do you expect a mole of ideal gas particles to ever undergo a spontaneous contraction in volume?
Transcribed Image Text:2) While water's boiling point at 1 atm is 100 °C, if you heat water quickly, you can "superheat" it past its boiling point. Superheated water is a kinetically metastable state and will rapidly boil if disturbed. a. Consider 13 mol of water (approximately 1 cup) that have been superheated to 110 °C. What is the enthalpy change for converting this superheated liquid into water vapor at 110 °C? To calculate this, you'll need to look up the heat capacity of water, the heat capacity of water vapor, and the enthalpy of vaporization of water. You can assume each of these quantities is constant over the range 100 110 °C. b. You should find your answer differs from that for vaporizing the same amount of water at 100 °C, water's normal boiling point. Can you provide a chemical explanation as to why these two quantities should differ? 3) What is the probability that 100 ideal gas particles will spontaneously contract their volume by 0.01%? What about 1000 ideal gas particles? How many molecules do you need to consider before the probability of contraction becomes less than 1%? Do you expect a mole of ideal gas particles to ever undergo a spontaneous contraction in volume?
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