Impossible tHERMODYNAMICS Problem

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SUMMARY

The discussion centers on a thermodynamics problem involving the latent heat of vaporization of water, specifically 2.26 × 106 J/kg. The problem requires calculating the work done when 9 grams of water transitions from liquid to vapor at one atmosphere, with a volume change from 0.5 cm3 to 2165 cm3. The work is calculated using the formula W = ΔV × P, where ΔV is the change in volume and P is the pressure. Participants express difficulty in unit conversions and calculations, prompting requests for detailed calculations.

PREREQUISITES
  • Understanding of latent heat and its application in phase changes
  • Knowledge of the ideal gas law and pressure-volume work
  • Familiarity with unit conversions, particularly between cm3 and m3
  • Basic principles of thermodynamics, including internal energy calculations
NEXT STEPS
  • Review the concept of latent heat and its role in phase transitions
  • Learn how to calculate work done in thermodynamic processes using W = ΔV × P
  • Study unit conversion techniques, especially for pressure and volume
  • Explore internal energy calculations in thermodynamic systems
USEFUL FOR

Students studying thermodynamics, physics enthusiasts, and anyone tackling problems related to phase changes and energy calculations in fluids.

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Homework Statement


Given: latent heat of vaporization of water = 2.26 × 106 J/kg .
Nine gram of water changes from liquid to vapor at a pressure of one atmosphere. In the process, the volume changes from 0.5 cm3 to 2165 cm3.
Find the work done. Answer in units of J.

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


Homework Equations



Latent Heat=2.26x10^6(kg)
this doesn't work

W=change in volume * pressure

The Attempt at a Solution


i have plugged in the values for the first section and they do not work. Changing to pascals/kg aren't right.
 
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Can you show your calculations in more detail, specifically the way you addressed the units?
 

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