From Robert Balmer\'s Modern Thermodynamics for Engineers, Chapter 7, Problem 29

Question

From Robert Balmer's Modern Thermodynamics for Engineers, Chapter 7, Problem 29

Determine the heat transport of entropy into a pan of boiling water at 100°C that has been sitting on a kitchen stove for 30.0 min. During this time, 0.300 kg of water is converted from a saturate liquid to a saturated vapor.

If someone could explain how to solve this, I would greatly appreciate it so I can solve similar problems on my own.

Thanks for any help. I'm more than happy to rate lifesaver for a complete response.

Explanation / Answer

latent heat of vaporization of water = L =2260 KJ/Kg

heat transferred = m.L = 0.3 x 2260 Kj

   Q = 678 KJ

entropy = Q/T

during boiling temp remains constant = 100 C = 373 K

hence, S = Q / T = 678 / 373

   = 1.817 KJ/Kg.K = entropy transferred to the pan

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