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During a strenuous workout, an athlete generates 2210 kJ of heat energy. What mass of water would have to evaporate from the athlete's skin to dissipate 2210kJ of heat?

During a strenuous workout, an athlete generates 2210 kJ of heat energy. What mass of water would have to evaporate from the athlete's skin to dissipate 2210kJ of heat?

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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At 100.0°C the molar heat of vaporization of water is 40.67 kJ/mol. At 25.0°C, approximately room temperature, the molar heat of vaporization of water is 44.0 kJ/mol. During a strenuous workout, an athlete generates 2210 kJ of heat energy. What mass of water would have to evaporate from the athlete's skin to dissipate 2210kJ of heat?
Transcribed Image Text:At 100.0°C the molar heat of vaporization of water is 40.67 kJ/mol. At 25.0°C, approximately room temperature, the molar heat of vaporization of water is 44.0 kJ/mol. During a strenuous workout, an athlete generates 2210 kJ of heat energy. What mass of water would have to evaporate from the athlete's skin to dissipate 2210kJ of heat?
L ou have un ea attempts/hereis no ar ant nenalty 131- The enthalpy change for the explosion of ammonium nitrate with fuel oil is -7198 kJ for every 3 moles of NH4NO3. What is the enthalpy change for 1.0 mole of NH4NO3 in this reaction? mnt kJ
Transcribed Image Text:L ou have un ea attempts/hereis no ar ant nenalty 131- The enthalpy change for the explosion of ammonium nitrate with fuel oil is -7198 kJ for every 3 moles of NH4NO3. What is the enthalpy change for 1.0 mole of NH4NO3 in this reaction? mnt kJ
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