Question

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∘.

Part A: Calculate the energy absorbed from a climber's body if he eats 0.50 kg of -15∘C snow which his body warms to body temperature of 37∘C. Express your answer to two significant figures and include the appropriate units.

Part B: Calculate the energy absorbed from a climber's body if he melts 0.50 kg of -15∘C snow using a stove and drink the resulting 0.50 kg of water at 2∘C, which his body has to warm to 37∘C. Express your answer to two significant figures and include the appropriate units.

Answer 1

Answer;;

a) The specific heat of ice is 2100 J/kg. C = S_ice

the latent heat of fusion is 333 KJ/kg = L_Ice

the specific heat of water is 4186 J/kg. C = S_water

  Calculate the energy absorbed from a climber's body if he eats 0.50 kg of -15∘C, where is 3 possible events

1)

eat required to change 0.50 kg ice at −15∘C to Ice at 0∘C

J

2) Heat required to change from state of 0.50  kg ice to water

  

3) Heat required to change 0.50 kg water at 0∘C to water at 37∘C

  

=

Total heat required= (15750 +166500 +77441) J

=337132 J

=3.38×10⁵ J

The answer is =3.38×10⁵ J

B)

Drink the resulting 0.50 kg of water at 2∘C, which his body has to warm to 37∘C.

  

  

   The answer is