Challenge Problem!!! Two 20.0 g ice cubes at -11.0 °C are placed into 245 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tr, of the water after all the ice melts. heat capacity of H₂O(s) heat capacity of H₂O(1) 37.7 J/(mol·K) 75.3 J/(mol-K) T₁ = enthalpy of fusion of H₂O 6.01 kJ/mol C
Challenge Problem!!! Two 20.0 g ice cubes at -11.0 °C are placed into 245 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tr, of the water after all the ice melts. heat capacity of H₂O(s) heat capacity of H₂O(1) 37.7 J/(mol·K) 75.3 J/(mol-K) T₁ = enthalpy of fusion of H₂O 6.01 kJ/mol C
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 88QRT: If you want to convert 56.0 g ice (at 0 °C) to water at 75.0 °C, calculate how many grams of...
Question

Transcribed Image Text:Challenge Problem!!! Two 20.0 g ice cubes at -11.0 °C are placed into 245 g of water at 25.0 °C. Assuming no energy is
transferred to or from the surroundings, calculate the final temperature, Tr, of the water after all the ice melts.
heat capacity of H₂O(s)
heat capacity of H₂O(1)
37.7 J/(mol·K)
75.3 J/(mol-K)
T₁ =
enthalpy of fusion of H₂O
6.01 kJ/mol
C
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