How much heat is required to heat 1 ton of water from 60 degrees Celsius (at a pressure of 2.65 MPa) to 250 degrees Celsius (at a pressure of 3.9 MPa)?
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Question: How much heat is required to heat 1 ton of water from 60 degrees Celsius (at a pressure of 2.65 MPa) to 250 degrees Celsius (at a pressure of 3.9 MPa)? How to calculate it?
This post was last edited by ylb913 on 2018-6-30 at 16:05. First of all, with the pressure increasing from 2.65 MPa to 3.9 MPa, heat should not need to be considered, right? This relies on a pump, and there is throttling at the pump outlet; the pressure at the pump outlet is far more than 3.9 MPa. The enthalpy change for 1 kg of water heated from 60 degrees Celsius (pressure of 3.9 MPA, absolute pressure) to 250 degrees Celsius (still at 3.9 MPA) is 2805.85 – 254.41 = 2551.44 KJ. For 1 ton, this amount is 2551440 KJ, or 610,400 kilocalories.
It is caused by the increase in pressure resulting from water absorbing heat
2805.85 - 253.36 = 2552.49 KJ; 1 ton is equivalent to 2,552,490 KJ, or 610,600 kilocalories.