Chemistry, 15.02.2021 04:40, zalayjahan4793
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: 2
Chemistry, 22.06.2019 17:30, mwest200316
To find the enthalpy of a reaction in the lab, you measured the of the reactants and the change during the reaction.
Answers: 1
Chemistry, 22.06.2019 21:30, kawaiiblurainbow
Which of the following changes will decrease the total amount of gaseous solute able to be dissolved in a liter of liquid water? (2 points) decreasing temperature decreasing pressure decreasing surface area decreasing solute concentration
Answers: 1
Chemistry, 22.06.2019 22:00, notearslefttocry14
Imagine one batch of soup (batch “a”) is made with 8.19 g/can of salt, according to the recipe, and a second batch of soup (batch “b”) is made with 8.32 g/can of salt. explain which batch would be more resistant to frost damage if it is shipped a great distance in winter and explain why.
Answers: 2
Evaporation of sweat requires energy and thus takes excess heat away from the body. Some of the wate...
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