Thermodynamics internal energy Problem

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SUMMARY

The discussion centers on calculating the increase in internal energy of water transitioning from liquid to vapor at one atmosphere. The latent heat of vaporization for water is specified as 2.26 × 10^6 J/kg. The user initially calculated the heat transfer using the formula Q = mL, resulting in an incorrect value of 13500 J. The correct approach requires accounting for the work done during the volume change from 0.9 cm³ to 2387 cm³, leading to a reevaluation of the internal energy increase.

PREREQUISITES
  • Understanding of thermodynamic principles, specifically internal energy and phase changes.
  • Familiarity with the concept of latent heat and its calculation.
  • Basic knowledge of the ideal gas law and work done during expansion.
  • Proficiency in using the formula Q = mL for heat transfer calculations.
NEXT STEPS
  • Study the first law of thermodynamics and its application in phase transitions.
  • Learn about calculating work done during volume changes in thermodynamic processes.
  • Explore the relationship between temperature, pressure, and volume in phase changes.
  • Investigate the latent heat values for other substances and their implications in thermodynamics.
USEFUL FOR

Students and professionals in physics and engineering, particularly those focusing on thermodynamics, heat transfer, and energy calculations in phase changes.

liamtcarroll
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Six grams of water changes from liquid to
vapor at a pressure of one atmosphere. In the
process, the volume changes from 0.9 cm^3
to2387 cm^3. The latent heat of vaporization of
water is 2.26 × 10^6 J/kg

Find the increase in internal energy of the
water.
Answer in units of J

When i did this i did Q=mL. I got 13500J to be my answer and the program I'm using said it was wrong
 
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I answered it myself i had to subtract my work from my answer
 

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