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Chemistry (181)
CHM 113 (103)
Ron Briggs (24)
Lecture

Enthalpy

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Department
Chemistry
Course
CHM 113
Professor
Ron Briggs
Semester
Fall

Description
Enthalpy of reaction - A state function, to determine ΔH , we don’t need to know the series of step a rxn reaction went though - Hess’ Law: If a reaction is carried out in a series of steps, ΔH rxnwill equal the sum of the ΔH’s for the individual steps o Example: To determine ΔH rxnfor: CH 4g) + 2O (2) → CO (g) 2 2H O (l) 2 o We can add up ΔH’s for other reactions already measured  CH 4g) + 2O (g2 → CO (g) +22H O (g) 2  ΔH = -802 kJ (Found Appendix C or page 184 of book)  2H 2(g) → 2H O(l2  ΔH = -88 kJ  Cancel out 2H O(g) on both sides of either reaction and form CH (g) + 2 4 2O 2g) → CO (g)2+ 2H O (l2  ΔH = -802 + -88 = -890kJ o
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