∆U = qV versus ∆H = qP | Lecture Note - Edubirdie

University:
Boston University
Course:
CAS CH 214 | Organic Chemistry with Qualitative Analysis
Academic year:

2024
Views:

355

Pages:

7
Author:

Annabel Combs

∆U = qV versus ∆H = qP ∆U = qV versus ∆H = qP ∆U = qV versus ∆H = qP Exothermic reaction that does work on surroundings will get hotter at constant volume. 2 ∆U = qV versus ∆H = qP ∆U = qV versus ∆H = qP Exothermic reaction that has work done on it will get less hot at constant volume. 3 ∆U = qV versus ∆H = qP ∆U = qV versus ∆H = qP Endothermic reaction that has work done on it will get colder at constant volume. 4 ∆U = qV versus ∆H = qP ∆U = qV versus ∆H = qP Endothermic reaction that does work on surroundings will get less cold at constant volume. 5 ∆U = qV versus ∆H = qP ∆U = qV versus ∆H = qP In a sealed, rigid container … constant V  no work possible  ∆T is a measure of ∆U = qV In an open container … constant P  work possible  ∆T is a measure of ∆H = qP Open container Gas moles |∆Tclose| > |∆Topen|? Exothermic Formed Greater (hotter) Exothermic Consumed Smaller (less hot) Endothermic Formed Smaller (less cold) Endothermic Consumed Greater (colder) 6 ∆U = qV versus ∆H = qP 7

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