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Chemical Thermodynamics 2013/2014

Chemical Thermodynamics 2013/2014. 4 th Lecture: Manipulations of the 1 st Law and Adiabatic Changes Valentim M B Nunes, UD de Engenharia. Relations between partial derivatives.

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Chemical Thermodynamics 2013/2014

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  1. ChemicalThermodynamics2013/2014 4th Lecture: Manipulations of the 1st Law and Adiabatic Changes Valentim M B Nunes, UD de Engenharia

  2. Relations between partial derivatives Partial derivatives have many useful properties, and we can use it to manipulate the functions related with the first Law to obtain very useful thermodynamic relations. Let us recall some of those properties. If f is a function of x and y, f = f(x,y), then If z is a variable on which x and y depend, then

  3. Relations between partial derivatives The Inverter: The Permuter: Euler’s chain relation: Finally, the differential df = g dx + h dy is exact, if:

  4. Changes in Internal Energy Recall that U = U(T,V). So when T and V change infinitesimally The partial derivatives have already a physical meaning (remember last lecture), so:

  5. Change of U with T at constant pressure What does this mean? Using the relation of slide 2 we can writhe: We define the isobaric thermal expansion coefficient as Finally we obtain: Closed system at constant pressure and fixed composition! = 0 for an ideal gas Proofs relation between Cp and Cv for an ideal gas!

  6. Change of H with T at constant volume Let us choose H = H(T,p). This implies that Now we will divide everything by dT, and impose constant volume What is the meaning of this two partial derivatives?

  7. Change of H with T at constant volume What does this mean? Using the Euler’s relation Rearranging We define now the isothermal compressibility coefficient To assure that kT is positive! So, we find that

  8. Change of H with T at constant volume Using again the Euler’s relation and rearranging or What is this? See next slide! For now we will call it µJT We finally obtain

  9. The Joule-Thomson Expansion Consider the fast expansion of a gas trough a throttle: If Q = 0 (adiabatic) then So, by the definition of enthalpy Isenthalpic process!

  10. The Joule-Thomson effect For an ideal gas, µJT = 0. For most real gases Tinv >> 300 K. If µJT >0 the gas cools upon expansion (refrigerators). If µJT <0 then the gas heats up upon expansion.

  11. Adiabatic expansion of a perfect gas From the 1st Law, dU = dq + dw. For an adiabatic process dU = dw and dU = CvdT, so for any expansion (or compression): For an irreversible process, against constant pressure: The gas cools!

  12. Adiabatic expansion of a perfect gas For a reversible process, CVdT = -pdV along the path. Now, per mole, for an ideal gas, PV = RT, so For an ideal gas, Cp-Cv = R, and introducing then The gas cools!

  13. Adiabatic expansion of a perfect gas We can now obtain an equivalent equation in terms of the pressure: As a conclusion, is constant along a reversible adiabatic. For instance, for a monoatomic ideal gas,

  14. Adiabatic vs isothermal expansion

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