Suppose you are overtaken by a blizzard while ski touring and you take refuge in a tent. You are thirsty, but you forgot to bring liquid water. You have a choice of eating a few handfuls of snow (say 400 g) at −5.0 °C immediately to quench your thirst or setting up your propane stove, melting the
Suppose you are overtaken by a blizzard while ski touring and you take refuge in a tent. You are
thirsty, but you forgot to bring liquid water. You have a choice of eating a few handfuls of snow (say
400 g) at −5.0 °C immediately to quench your thirst or setting up your propane stove, melting the
snow, and heating the water to body temperature before drinking it. You recall that the survival guide you leafed through at the hotel said something about not eating snow, but you cannot
remember why–after all, it’s just frozen water. To understand the guide’s recommendation, calculate
the amount of heat that your body will have to supply to bring 400. g of snow at −5.0 °C to your
body’s internal temperature of 37 °C. The specific heats of liquid water and ice are 4.184 J/(g•°C) and
2.062 J/(g•°C), respectively, and the enthalpy of fusion of ice is 6.01 kJ/mol.
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