Chemistry 12th Edition

Published by McGraw-Hill Education
ISBN 10: 0078021510
ISBN 13: 978-0-07802-151-0

Chapter 6 - Thermochemistry - Questions & Problems - Page 263: 6.24

Answer

We find: a) $\Delta$H = $2 (-1452.8kJ/mol) = -2905.5 kJ/mol$ b) $\Delta$H = $- (-1452.8kJ/mol) = 1452.8 kJ/mol$ a) $\Delta$H = $ -1452.8kJ/mol -(4mol)(-285.8kJ/mol) + (4mol)(-242kJ/mol) = -1277.6 kJ/mol$

Work Step by Step

We find: a) $\Delta$H = $2 (-1452.8kJ/mol) = -2905.5 kJ/mol$ b) $\Delta$H = $- (-1452.8kJ/mol) = 1452.8 kJ/mol$ a) $\Delta$H = $ -1452.8kJ/mol -(4mol)(-285.8kJ/mol) + (4mol)(-242kJ/mol) = -1277.6 kJ/mol$
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