Question
2. Consider the oxidation of nitric oxide to produce nitrogen dioxide: 2 NO ( g ) + O 2 ( g ) 2 NO
2. Consider the oxidation of nitric oxide to produce nitrogen dioxide: 2 NO (g) + O2 (g) → 2 NO2 (g)
a) Use the following data to calculate ΔHrxn for this process.
N2 (g) + O2 (g) → 2 NO (g) ΔH = + 180.5 kJ
N2 (g) + 2 O2 (g) → 2 NO2 (g) ΔH = + 66.4 kJ
b) Enthalpy is a state function. What does this mean and why is it important for answering the question in part a?
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Elementary Principles of Chemical Processes
Authors: Richard M. Felder, Ronald W. Rousseau
3rd Edition
978-0471687573, 9788126515820, 978-0-471-4152, 0471720631, 047168757X, 8126515821, 978-0471720638
