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LEC 02 CHAP 07 - Lecture 2 Internal Energy First Law of...

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TOUPADAKIS Chapter 7 Lecture 2 Lecture 2 Internal Energy First Law of Thermodynamics State Functions versus Path Functions Heat Transfer during a Physical Change Heat Transfer During a Chemical Change At constant volume (q v ) At constant pressure (q p ) Standard State and Standard Enthalpy of a Reaction
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TOUPADAKIS Chapter 7 Lecture 2 Internal Energy (U) The total energy of a system (potential and kinetic) on the microscopic scale . •Translational kinetic energy. •Rotational kinetic energy. •Vibrational kinetic energy. •Potential energy due to intermolecular attractions. •Potential energy due interatomic attractions. •Potential energy due to attractions between electrons and nuclei. •Potential energy due to attractions between the components of the nuclei.
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TOUPADAKIS Chapter 7 Lecture 2 First Law of Thermodynamics For an isolated system the change of its internal energy is zero: (internal energy is constant) Δ U = 0 For a closed system the change of its internal energy is: Δ U = (±q) + ( ± w)
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TOUPADAKIS Chapter 7 Lecture 2 Problem 1 First Law of Thermodynamics During an endothermic process 15.6 kJ of energy in the form of heat was transferred between a closed system and its surroundings.
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