Solution Found!
Answer: (a) Calculate the change in entropy when 1.00 kg
Chapter 20, Problem 29E(choose chapter or problem)
Problem 29E
(a) Calculate the change in entropy when 1.00 kg of water at \(100^{\circ} \mathrm{C}\) is vaporized and converted to steam at \(100^{\circ} \mathrm{C}\) (see Table 17.4). (b) Compare your answer to the change in entropy when 1.00 kg of ice is melted at \(0^{\circ} \mathrm{C}\), calculated in Example 20.5 (Section 20.7). Is the change in entropy greater for melting or for vaporization? Interpret your answer using the idea that entropy is a measure of the randomness of a system.
Equation Transcription:
Text Transcription:
100degC
100degC
0degC
Questions & Answers
QUESTION:
Problem 29E
(a) Calculate the change in entropy when 1.00 kg of water at \(100^{\circ} \mathrm{C}\) is vaporized and converted to steam at \(100^{\circ} \mathrm{C}\) (see Table 17.4). (b) Compare your answer to the change in entropy when 1.00 kg of ice is melted at \(0^{\circ} \mathrm{C}\), calculated in Example 20.5 (Section 20.7). Is the change in entropy greater for melting or for vaporization? Interpret your answer using the idea that entropy is a measure of the randomness of a system.
Equation Transcription:
Text Transcription:
100degC
100degC
0degC
ANSWER:
Solution to 29E
Step 1
When the water reaches the boiling point at T=373.15K, it changes into steam and the temperature will keep constant until water is completely transformed into steam. Thus, conversion of water into steam is a isothermal process.
Mass of water =1kg
Latent heat of vaporization of water =2.256x106K/kg