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 500.mL of water equivalent to 500. g of water)that had been in the refrigerator at 3.8 °C, how much heat is needed to convert all of the 500.g of water into sweat and then to vapor?For the purpose of solving this problem, assume that the thermal properties of sweat are the same as for water. Thus, you are looking for the heat value to raise the temp of the liquid water from 3.8 °C to 100. °C and then vaporize that 500.g of water. Your final answer should be in kcal or MJ
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 500.mL of water equivalent to 500. g of water)that had been in the refrigerator at 3.8 °C, how much heat is needed to convert all of the 500.g of water into sweat and then to vapor?For the purpose of solving this problem, assume that the thermal properties of sweat are the same as for water. Thus, you are looking for the heat value to raise the temp of the liquid water from 3.8 °C to 100. °C and then vaporize that 500.g of water. Your final answer should be in kcal or MJ
There are two different heats that need to be calculated. For this purpose, the human body temperature is assumed to be . The different heats are:
- q1 for raising the temperature of water from to
- q2 for evaporating the steam at
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