Chemistry
9th Edition
ISBN: 9781133611097
Author: Steven S. Zumdahl
Publisher: Cengage Learning
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Chapter 10, Problem 119AE
In regions with dry climates, evaporative coolers are used to cool air. A typical electric air conditioner is rated at 1.00 × 104 Btu/h (1 Btu, or British thermal unit = amount of energy to raise the temperature of 1 lb water by 1°F). What quantity of water must be evaporated each hour to dissipate as much heat as a typical electric air conditioner?
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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.
Cs, liquid water
4.184 J/g °C
Cs,
1.84 J/g °C
%3D
steam
Cs, ice = 2.09 J/g °C
%3D
AHvap = 40.67 kJ/mol at 36.6 °C.
AHfus = 6.01 kJ/mol
%3D
1413 kJ
81 kJ
1150 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
%3D
Csteam= 1.84 J/g °C
Cice = 2.09 J/g °C
AHvap = 40.67 kJ/mol at 36.6 °C.
AHfus = 6.01 kJ/mol
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
cice = 2.09 J/g °C
ΔHvap = 40.67 kJ/mol at 36.6 °C.
ΔHfus = 6.01 kJ/mol
Chapter 10 Solutions
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- 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 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 oc. For the purpose of solving this problem, assume that the thermal properties of sweat are the same as for water.)arrow_forwardIf 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?arrow_forwardThe amount of heat required to melt 2 lbs of ice is twice the amount of heat required to melt 1 lb of ice. Is this observation a macroscopic or microscopic description of chemical behavior? Explain your answer.arrow_forward
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