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Unformatted text preview: Lecture 16 — Internal energy For a system of a single component, U must be a function of T,P (or T,v or P,v ), since there are only two independent state functions Expand the di ff erential of this state function, then, in T and v : dU = ( ∂ U/ ∂ T ) V dT + ( ∂ U/ ∂ V ) T dV Heat capacity. The first of these is C v , measured with calorimeter. Extensive or intensive, depend- ing on whether or not we made U intensive. Measurable, evidently, and a state function (since it’s the derivative of a state function). (How does a calorimeter work? Need a gadget for measuring temperature, and a calibrated source of heat. So we have dU = dQ , and we measure dT . Can calibrate a source of heat against a “mechanical work” source of heat.) If we have a constant-volume process, then, Δ U = T 2 T 1 C v ( T ) dT How does C v depend on T ? Molar heat capacity, C v /N ; how do liquids and gases compare? Liquids typically higher, because some of the heat energy is “stored” in disrupting the attractions between molecules. Example: compare C v /N for ideal gas and typical liquid....
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This note was uploaded on 04/01/2008 for the course CHE 220 taught by Professor Prof.marannas during the Spring '08 term at Penn State.
- Spring '08