Two 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H,0(s) 37.7 J/(mol-K) Tf = °C heat capacity of H,O(1) 75.3 J/(mol-K) enthalpy of fusion of H,O 6.01 kJ/mol

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter10: Liquids And Solids
Section: Chapter Questions
Problem 104E: A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice,...
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Two 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature, T;, of the water after all the ice melts.
heat capacity of H,O(s)
37.7 J/(mol·K)
Tf =
heat capacity of H,O(l)
75.3 J/(mol-K)
enthalpy of fusion of H,O
6.01 kJ/mol
Transcribed Image Text:Two 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T;, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/(mol·K) Tf = heat capacity of H,O(l) 75.3 J/(mol-K) enthalpy of fusion of H,O 6.01 kJ/mol
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