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Lecture-27 - Chem111 Fall 2005 Lecture 27 Thermodynamics...

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Chem111 Fall, 2005 thermo-7 Let's continue talking about heat and work … We said last time that The heats measured at constant volume and constant pressures are given by q V = n c V Δ T q P = n c P Δ T These heats can be correlated with thermodynamic state functions: q V = Δ E q P = Δ H Recall that c V and c P are molar heat capacities … can we come up with some (easy) expressions for these? For an ideal gas, we also know that KE = n 3/2 RT (n = # moles of gas) If the gas is monoatomic (e.g. neon, helium, argon, etc.) then there is no other place for energy that we put into the system to go! It just goes into the kinetic energy of the particles, and so we can say that Δ E = n 3/2 RT f – n 3/2 RT i = n 3/2 R Δ T Comparison to the above expression for q V shows that c V = 3/2 R Note: for gases that have more than one atom, c V > 3/2 R Lecture 27: Thermodynamics Heat and Work First Law of Thermodynamics
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Chem111 Fall, 2005 thermo-8 Let's look at our cylinder with a freely sliding piston again. This system starts out with 0.201 moles of neon gas in a volume of 5.00 L under a pressure of 1.00 atm.
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