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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.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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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.
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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