Essential University Physics: Volume 1 (4th Edition)

Published by Pearson
ISBN 10: 0-134-98855-8
ISBN 13: 978-0-13498-855-9

Chapter 17 - For Thought and Discussion - Page 324: 8


It takes more heat to boil the water.

Work Step by Step

First, recall that the heat required to melt ice is $334 KJ/kg$. Since there is a gram of ice, it will take: $\frac{334}{1000} = .334 kJ$. Now, we consider the specific heat of water to see how much energy it takes to increase the temperature of water by 100 Kelvin: $ Q = mC \Delta t \\ Q = (.001)(4.184)(100) = .4184 kJ$ This is more energy than melting the ice, so it will take more energy to boil water.
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