Determination of the final temperature inside a calorimeter

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SUMMARY

The discussion focuses on calculating the final temperature inside a calorimeter when a heated piece of copper (Cu) is introduced to water. A 5.33g piece of Cu at 372.85K is placed in 99.53g of water at 295.75K. The specific heat capacities are given as Cp[Cu(s)]=0.385 J/g*K and Cp[water]=4.184 J/g*K. The key formula used is (T2-T1)*Cp*m = Q, which establishes that the heat lost by the Cu equals the heat gained by the water, allowing for the determination of the final temperature and subsequent entropy changes.

PREREQUISITES
  • Understanding of specific heat capacity and its application in calorimetry.
  • Knowledge of the first law of thermodynamics regarding heat transfer.
  • Familiarity with the concept of entropy and its calculation.
  • Basic algebra skills for solving equations involving temperature and heat transfer.
NEXT STEPS
  • Study the principles of calorimetry and heat transfer in closed systems.
  • Learn how to calculate entropy changes for different materials.
  • Explore the application of the first law of thermodynamics in thermal equilibrium problems.
  • Practice solving calorimetry problems involving multiple substances and phase changes.
USEFUL FOR

This discussion is beneficial for chemistry students, particularly those studying physical chemistry, as well as educators and anyone interested in thermodynamic principles and calorimetry calculations.

soaring206
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Okay, I'm working on some pchem problems and I'm stuck on this one question...

A 5.33g piece of Cu metal is heated to 372.85K in boiling water, then dropped into a calorimeter containing 99.53g of water at 295.75K. The calorimeter is sealed to the outside environment, and the temperature equalizes. Cp[Cu(s)]=0.385 J/g*K, Cp[water]=4.184 J/g*K. What is the final temperature inside the system? What is the entropy change of the Cu metal? What is the entropy change of the liquid water? What is the total entropy change in the system?

I have absolutely no idea how to find the final temp of the system. Once I have that temp, I think I can figure out the entropy changes, but if someone could point me in the right direction for finding the final temperature, that would be great. Thank you in advance!
 
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Hint: (T2-T1)*Cp*m = Q. The heat lost by the Cu must equal the heat gained by the H2O.
 
Thanks, that helped a lot...I think I've figured it out now! :smile:
 

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