High-altitude mountain climbers do not eat snow, but always melt it first with a stove. To see why, calculate the energy absorbed from a climber's body under the following conditions. The specific heat of ice is 2100 J/kg⋅C∘, the latent heat of fusion is 333 kJ/kg, the specific heat of water is 4186 J/kg⋅C∘

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High-altitude mountain climbers do not eat snow, but always melt it first with a stove. To see why, calculate the energy absorbed from a climber's body under the following conditions. The specific heat of ice is 2100 J/kg⋅C∘, the latent heat of fusion is 333 kJ/kg, the specific heat of water is 4186 J/kg⋅C∘

a) eat 1.0kg of -15 degrees Celsius snow which your body warms to body temperature of 37 degrees Celsius ?

b) melt 1.0kg of -15 degrees Celsius snow using a stove and drink the resulting 1.0kg of water at 2 degrees Celsius, which your body has to warm to 37 degrees Celsius ?

Explanation:

Let's calculate the heat required to convert ice from -15°C to 0°C and then the heat required to convert it into the water.

a)

Heat required to convert -15°C ice to 0°C.

  ΔT = (1.0)(2.100×10³)(15) = 3.150×J

Heat required to convert 1.0 kg ice to water.

    ×× = 3.33×J

Heat required to convert 1.0 kg water at 0°C to 37°C.

   ΔT = 1×4.186××37 = 1.548× J

Total heat required = 3.150× + 3.33× + 1.548×

                              = 5.19× J

b)

Heat required to warm 1.0 kg water at 2°C to water at 37°C.

ΔT = 1×4.186××35

                = 1.465×J

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