For water, ΔHfusion = 6.02 kJ/mol and ΔHvap = 40.65 kJ/mol. If 0.250 moles of water vaporizes at 100 oC due to heat from the surroundings that are at 135 oC, what is the change in entropy in the surroundings?
For water, ΔHfusion = 6.02 kJ/mol and ΔHvap = 40.65 kJ/mol. If 0.250 moles of water vaporizes at 100 oC due to heat from the surroundings that are at 135 oC, what is the change in entropy in the surroundings?
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.10QE: Explain why absolute enthalpies and energies cannot be measured, and only changes can be determined.
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For water, ΔHfusion = 6.02 kJ/mol and ΔHvap = 40.65 kJ/mol. If 0.250 moles of water vaporizes at 100 oC due to heat from the surroundings that are at 135 oC, what is the change in entropy in the surroundings?
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