In the first stage of the industrial production of nitric acid, ammonia reacts at high temperature with oxygen in a reversible, exothermic reaction: 4 NH3(g) + 5 0₂(g) 4 NO(g) + 6H₂O(g) a) Predict the sign of the system entropy change in this reaction and explain your answer.
In the first stage of the industrial production of nitric acid, ammonia reacts at high temperature with oxygen in a reversible, exothermic reaction: 4 NH3(g) + 5 0₂(g) 4 NO(g) + 6H₂O(g) a) Predict the sign of the system entropy change in this reaction and explain your answer.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter13: Spontaneous Processes And Thermodynamic Equilibrium
Section: Chapter Questions
Problem 20P
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Transcribed Image Text:In the first stage of the industrial production of nitric acid, ammonia reacts at high temperature
with oxygen in a reversible, exothermic reaction:
4 NH3(g) + 5 0₂(g)
4 NO(g) + 6 H₂O(g)
a) Predict the sign of the system entropy change in this reaction and explain your answer.
b) Thermochemical data for this reaction are shown below. Use this data to determine the
system entropy change.
NH3(g)
192.3
-45.9
O₂(g)
205.0
0.0
NO(g)
210.7
90.2
H₂O(g)
+188.7
-285.8
Sº / J mol-1 K-1
H₂/kJ mol-¹
c) Use the values in the table to calculate the system standard enthalpy change, AH.
d) Use your answers to (b) and (c) to explain why this reaction is feasible at any temperature.
e) Use your answer to (c) to calculate the surroundings entropy change in J.mol-¹ K-¹ at 298K.
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