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September 19, 2014

September 19, 2014

Posted by **Amy** on Sunday, January 6, 2013 at 1:03pm.

If no heat is lost to the surroundings, what will be the final temperature of the mixture?

- What is the Final Temperature? -
**drwls**, Sunday, January 6, 2013 at 1:38pmTo melt all of the ice, 53*80= 4250 calories must be added. Cooling 120 g of water from 77 to 0 C would release 77*120 = 9240 calories. So all of the ice will melt. For the final temperature, set the heat lost by water equal to the heat gained by ice, including melted ice, and solve for T.

120*(77 - T) = 53* (80 + T)

Solve for T.

- What is the Final Temperature? -
**Amy**, Sunday, January 6, 2013 at 6:26pmI tried solving for T. I got 28.90 as my answer. It was still incorrect.

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