Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 5 - Thermochemistry - Exercises: 5.55a

Answer

6.772 kJ

Work Step by Step

There are 100g of water in the calorimeter and the temperature rises from 21.6 to 37.8 C. The specific heat of water is 4.18 J/g*K so first we need to find the $\Delta T = 37.8 - 21.6 = 16.2 C $. Since a $\Delta T$ of 1 C is equivalent to a change of 1K then we can write 16.2C as 16.2K. Then, to find how much energy is released we do the following: 4.18 J/g*K * 100g * 16.2K = 6771.6 J Then to convert to kJ we divide by 1000: 6.772 kJ
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