4. For the irreversible transition of: 100 g H20 (s, -25°C) 100 g H2O (v, +120°C

Question

4. For the irreversible transition of: 100 g H20 (s, -25°C) 100 g H2O (v, +120°C) Calculate the total amount of heat necessary to effect a set of reversible reactions for theses conditions. 5. In a steam radiator, steam at 110°C condenses and the liquid water formed is cooled to 80°C. How much heat per gram of liquid formed, is released in this process? 6. How much heat is absorbed by a persons hand if 100 grams of liquid water at 100°C is poured on his hand? (Assume the final temperature of the water will be normal body temperature of 37°C)

Explanation / Answer

6)

Given

Mass of water = 100 g

Intial temperature = 100 C

Final temperature = 37 C

Cp of water = 4 J/g.C

heat absorbed by the body = - heat lost by water = - m * Cp * ( T2 - T1) = - 100 g * 4 J/g.C ( 37 - 100) C = 25200 J

Answer persons hand will absorb 25.2 kJ  

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