H2(g) + F2(g) → 2 HF(g) ΔH = -542 kJ What would be the enthalpy change for the reverse of the given equation (that is, for the decomposition of HF into its constituent elements)?
H2(g) + F2(g) → 2 HF(g) ΔH = -542 kJ What would be the enthalpy change for the reverse of the given equation (that is, for the decomposition of HF into its constituent elements)?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter8: Thermochemistry
Section: Chapter Questions
Problem 36QAP: Given the following thermochemical equations: 4B(s)+3O2(g)2B2O3(s)H=2543.8kJ H2(g)+12...
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H2(g) + F2(g) → 2 HF(g) ΔH = -542 kJ
What would be the enthalpy change for the reverse of the given equation (that is, for the decomposition of HF into its constituent elements)?
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