Thermodynamics Energy when flashing water -- How much water will be vaporized?

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SUMMARY

The discussion focuses on calculating the amount of water vaporized during a flashing process at 75 degrees Celsius, with post-flash cooling to 67 degrees Celsius and a constant pressure of 0.27 bar. The flow rate is specified at 15,000 kg per hour. The participants emphasize the need for applying thermodynamic principles, particularly the use of steam tables and energy balance equations, to derive the vaporization quantity accurately.

PREREQUISITES
  • Understanding of thermodynamic principles, specifically phase changes.
  • Familiarity with steam tables for water at varying pressures and temperatures.
  • Knowledge of energy balance equations in thermodynamic systems.
  • Ability to perform calculations involving mass flow rates and enthalpy changes.
NEXT STEPS
  • Study the properties of water and steam using steam tables at various pressures.
  • Learn how to apply the first law of thermodynamics to phase change problems.
  • Research the concept of flashing in thermodynamics and its applications.
  • Explore examples of energy balance calculations in industrial processes.
USEFUL FOR

Engineers, thermodynamics students, and professionals involved in process design or energy management who require a deeper understanding of phase changes in water and vaporization calculations.

Keeskwaak
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TL;DR
Thermodynamics Energy, flashing water how much water will be vaporized
Hello all,
For a project I really need to know some number i can't seem to produce myself.

we are flashing water @75 degrees Celsius, the water after flash-cooling is 67 degrees constant pressure is 0.27 bar (absolute) flow rate is 15000 KG/per hour.

how much water is vaporized?

Help is much appreciated
 
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Please repost this in the homework help section, and follow the template/show your work (even if not actual homework it is a homework type problem). Thanks, thread locked.
 

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