Calorimetry Help: Solving a Problem with Ice Phase Change

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To calculate the final temperature after mixing 250 mL of coffee at 80 degrees C with 250 g of ice at 0 degrees C, it’s essential to consider the heat transfer involved in the phase change of ice. The heat of fusion for ice is 6.01 kJ/mol, indicating that this amount of energy is required to melt 1 mol of ice at 0 degrees C into water at the same temperature. The discussion emphasizes the importance of showing work for clarity in problem-solving. Participants encourage providing details of any calculations already attempted to facilitate further assistance. Understanding the heat transfer dynamics is crucial for determining the final temperature accurately.
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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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