Chemistry: The Central Science (13th Edition)

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

Chapter 5 - Thermochemistry - Exercises - Page 206: 5.48a


$\Delta H $ = -630 kJ

Work Step by Step

C6H6 --> 3 C2H2 $\Delta H = + 630 kJ $ If we want to find the enthalpy change for the reverse reaction, we would need to multiply the enthalpy by negative 1 since we are reversing the direction. This means $\Delta H $ = -1 * 630kJ = -630 kJ
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