Evaporation of sweat requires energy and thus takes 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 °C. For the
purpose of solving this problem, assume that the thermal properties of sweat are
the same as for water.)
Design a plan to solve this problem. What must be considered in order to solve
this? Explain it in words. Actual calculations are not needed, but can be included.
Answers: 1
Chemistry, 21.06.2019 21:30
It takes 945.kj/mol to break a nitrogen-nitrogen triple bond. calculate the maximum wavelength of light for which a nitrogen-nitrogen triple bond could be broken by absorbing a single photon.
Answers: 3
Chemistry, 22.06.2019 12:30
Suppose you wanted to make 100 grams of water. what is the molar mass of water (h2o)?
Answers: 2
Chemistry, 22.06.2019 14:40
Choose an equation that represents an enzyme-catalyzed reaction. (a) enzyme + substrate → enzyme-substrate complex (b) enzyme + substrate ←−→ enzyme + products (c) enzyme + substrate ←−→ enzyme-substrate complex → enzyme + products (d) enzyme + substrate ←−→ enzyme-substrate complex → enzyme-substrate complex + products
Answers: 2
Evaporation of sweat requires energy and thus takes excess heat away from
the body. Some of the wat...
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