Physical Chemistry I (TKK-2246)

1. 13/14 Semester 2 Physical Chemistry I(TKK-2246) Instructor: Rama Oktavian Email: rama.oktavian86@gmail.com • Office Hr.: M.13-15, Tu. 13-15, W. 13-15, Th. 13-15, F. 09-11

2. Outlines 1. Change in energy 2. Change in state at constant volume 3. Change in state at constant pressure 4. Adiabatic change state (Process calculation in ideal gas)

3. Change in energy Energy is an extensive state property of the system Energy per mole is an intensive state property of the system Energy is conserved in all transformations First law thermodynamic dU = dQ + dW dU of the system depends only onthe initial and final states Q and W depends on path

4. Change in energy First law thermodynamic dU = dQ + dW dU of the system depends only onthe initial and final states. Define U = U(T,V) Substituting dU from the first law thermodynamic

5. Change in energy First law thermodynamic

6. Change in energy First law thermodynamic

7. Change in energy First law thermodynamic This is the general first-law equation for a mechanically reversible, closed-system process

8. Change in energy Example of energy change – state and path function

9. Change in state at constant volume First law thermodynamic Change state at constant volume

10. Change in state at constant volume New properties – heat capacity Heat capacity at constant volume

11. Change in state at constant volume Heat calculation at constant volume If Cv constant

12. Change in state at constant volume Heat calculation at constant volume Valid for constant volume process Heat calculation at constant volume process

13. Change in state at constant pressure In laboratory practice most changes in state are carried out under a constant atmospheric pressure

14. Change in state at constant pressure Recall first law thermodynamics mathematical formulation Integrating this equation at constant pressure, we obtain

15. Change in state at constant pressure Rearranging this equation

16. Change in state at constant pressure Introducing new extensive state property of system Enthalpy Valid for constant-pressure process

17. Change in state at constant pressure Heat calculation at constant pressure process constant pressure process

18. Change in state at constant pressure Heat calculation at constant pressure process Heat capacity at constant pressure process If Cp is constant Valid for constant pressure process

19. Implied property relation for ideal gas Relation between Cv and Cp

20. Adiabatic change Adiabatic – no heat flow the first law statement is

21. Adiabatic change Adiabatic change state in ideal gas For ideal gas

22. Adiabatic change Integrating this equation from initial state (T1, V1) into final state (T2, V2), we have If Cv is independent to temperature (T)

23. Adiabatic change For ideal gas we have relationship

24. Adiabatic change PVT relationship for adiabatic change state in gas ideal

25. Adiabatic change Adiabatic change PV-graph

26. Learning check Check and Re-do example 7.3 from Castellan An ideal gas, Cv = 5/2 R, is expanded adiabatically against a constantpressure of 1 atm until it doubles in volume. If the initial temperature is 25 °C, andthe initial pressure is 5 atm, calculate T2 ; then calculate Q, W, ΔU, and ΔH per mole of gas for the transformation.

27. Assignment Open your textbook (Castellan) and do these following problem: Problem 7.1, 7.4, 7.10, 7.15, 7.17 The constant-pressure heat capacity of a sample of a perfect gas wasfound to vary with temperature according to the expression Cp /(J K−1) =20.17 + 0.4001(T/K). Calculate q, w, ΔU, and ΔH when the temperature israised from 0°C to 100°C (a) at constant pressure, (b) at constant volume.

28. Process in ideal gas Isothermal Process (constant temperature) for closed system process Governing equation

29. Process in ideal gas Isobaric Process (constant pressure) for closed system process

30. Process in ideal gas Isochoric Process (constant volume) for closed system process

31. Process in ideal gas Example

32. Thank You !