In a reaction, 1.00 mole of H2 is produced at a constant pressure of 1.00 atm and at 298 K (1 L atm = 101.3 J): 2 H2O(g) → 2 H2(g) + O2(g) ΔH° = +483.6 kJ mol–1 What is ΔE in this reaction? +243.0 kJ +240.6 kJ +239.3 kJ
In a reaction, 1.00 mole of H2 is produced at a constant pressure of 1.00 atm and at 298 K (1 L atm = 101.3 J): 2 H2O(g) → 2 H2(g) + O2(g) ΔH° = +483.6 kJ mol–1 What is ΔE in this reaction? +243.0 kJ +240.6 kJ +239.3 kJ
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 42QRT
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In a reaction, 1.00 mole of H2 is produced at a constant pressure of 1.00 atm and at 298 K (1 L atm = 101.3 J):
2 H2O(g) → 2 H2(g) + O2(g) ΔH° = +483.6 kJ mol–1
What is ΔE in this reaction?
|
+243.0 kJ |
|
+240.6 kJ |
|
+239.3 kJ |
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