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
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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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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