FOUNDATIONS OF COLLEGE CHEM +KNEWTONALTA
FOUNDATIONS OF COLLEGE CHEM +KNEWTONALTA
15th Edition
ISBN: 9781119797807
Author: Hein
Publisher: WILEY
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Chapter 13, Problem 24RQ
Interpretation Introduction

Interpretation:

Whether ice at 0 °C or water at 0 °C has less energy has to be determined.

Concept Introduction:

Heat of fusion is amount of heat required to convert solid to liquid. Every substance has different heat of fusion. Heat of fusion for ice is 384 J/g. It is represented as ΔHfus.

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A 22.5-g sample of ice at 0.0°C is added to 100.0 g of warm water at 35.0°C, and the final temperature of the mixture is 14.0°C. (a) How much heat (in Joules) is lost by the warm water? (b) How much heat (in Joules) is absorbed by the melted ice when its temperature increases from 0.0°C to 14.0°C? (c) How much heat is absorbed by ice during melting at 0.0°C? (d) What is the enthalpy of fusion of ice in kJ/mol? 3. (Specific heat of water = 4.184 J/(g.°C)

Chapter 13 Solutions

FOUNDATIONS OF COLLEGE CHEM +KNEWTONALTA

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