Chemistry: The Central Science (13th Edition)

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

Chapter 5 - Thermochemistry - Exercises: 5.26b


$\Delta E = +322 J$ Endothermic

Work Step by Step

The bar of gold absorbs 322J of heat. Since it is absorbing heat, heat is entering the system, so it is positive. This means that q = + 322J. Since $\Delta E = q + w$ then we have $\Delta E = +322J + 0 = 322 J $ Since this is positive, it means it is endothermic
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