A student performs the Determining the Heat of Fusion of Water experiment and obtains the following data. 5.6125 mass of empty calorimeter (g): mass of calorimeter with hot water (g): hot water temperature just before adding ice ('C): 68.0 lowest water temperature ("C): mass of calorimeter with cooled water (g): 54.5878 5.2 93.6000 Calculate the heat lost by the liquid water. Hint: If heat is lost, what should be the sign of q? Report your answer in kJ to one decimal place.
A student performs the Determining the Heat of Fusion of Water experiment and obtains the following data. 5.6125 mass of empty calorimeter (g): mass of calorimeter with hot water (g): hot water temperature just before adding ice ('C): 68.0 lowest water temperature ("C): mass of calorimeter with cooled water (g): 54.5878 5.2 93.6000 Calculate the heat lost by the liquid water. Hint: If heat is lost, what should be the sign of q? Report your answer in kJ to one decimal place.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 64E: A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed...
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Transcribed Image Text:A student performs the Determining the Heat of Fusion of Water experiment and
obtains the following data.
mass of empty calorimeter (g):
mass of calorimeter with hot water (g):
hot water temperature just before adding ice ("C): 68.0
lowest water temperature ("C):
mass of calorimeter with cooled water (g):
5.6125
54.5878
5.2
93.6000
Calculate the heat lost by the liquid water. Hint: If heat is lost, what should be the
sign of q? Report your answer in kJ to one decimal place.
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