Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the water that you drink may eventually be converted into sweat and evaporate. If you drink a 20-ounce bottle of water (590g) that had been in the refrigerator at 3.8 °C, how much heat is needed to convert all of that water into sweat and then to vapor? (Note: Your body temperature is 36.6 °C. For the purpose of solving this problem, assume that the thermal properties of sweat are the same as for water. Cliquid water = 4.184 J/g °C Csteam= 1.84 J/g °C %3D Cice = 2.09 J/g °C AHvap = 40.67 kJ/mol at 36.6 °C. %3D AHfus = 6.01 kJ/mol %3D 1536 kJ 1414 kJ 141.4 kJ 2530 kJ

Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the water that you drink may eventually be converted into sweat and evaporate. If you drink a 20-ounce bottle of water (590g) that had been in the refrigerator at 3.8 °C, how much heat is needed to convert all of that water into sweat and then to vapor? (Note: Your body temperature is 36.6 °C. For the purpose of solving this problem, assume that the thermal properties of sweat are the same as for water. Cliquid water = 4.184 J/g °C Csteam= 1.84 J/g °C %3D Cice = 2.09 J/g °C AHvap = 40.67 kJ/mol at 36.6 °C. %3D AHfus = 6.01 kJ/mol %3D 1536 kJ 1414 kJ 141.4 kJ 2530 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...

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