Calorimetry Help: Solving a Problem with Ice Phase Change

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SUMMARY

The discussion centers on calculating the final temperature after mixing 250 mL of coffee at 80 degrees Celsius with 250 g of ice at 0 degrees Celsius. The heat of fusion for ice is established as 6.01 kJ/mol, indicating that 6.01 kJ of heat is required to melt 1 mol of ice at 0 degrees Celsius. Participants emphasize the importance of demonstrating preliminary work to receive further assistance in solving the problem effectively.

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  • Understanding of calorimetry principles
  • Knowledge of heat transfer and phase changes
  • Familiarity with the concept of heat of fusion
  • Basic algebra for solving equations
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  • Learn about the specific heat capacities of water and coffee
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This discussion is beneficial for students studying thermodynamics, educators teaching calorimetry, and anyone interested in understanding heat transfer during phase changes.

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I needed to know if anyone can help me solve a problem.

I am supposed to calculate the final temperature after mixing 250 mL of coffee at 80 degrees C with 250 g of ice at 0 degrees C.

The heat of fusion for ice is 6.01 kJ/mol

The ice undergoes a phase change, but I don't know how to apply it. Can anyone help me?
 
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Well the heat of fusion says it all. It is 6.01 kJ/mol. That means that it takes 6.01 kJ of heat to melt 1 mol of ice--that is changing 1 mol of ice at 0 degrees C to 1 mol of water at 0 degrees C.

Technically you're supposed to show some work before you can get help here, so if you need more help please post to what extent you've worked the problem out so far.
 
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