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

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

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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