1. Chapter 2 The First Law Unit 4 thermochemistry
Spring 2009

2. Thermochemistry
The study of the energy transferred as heat during the course of chemical reactions is called thermochemistry.

3. Thermochemistry
we can use calorimetry to measure the energy supplied or discarded as heat by a reaction.
We can identify q with a change in internal energy DU (if the reaction occurs at constant volume) or a change in enthalpy DH (if the reaction occurs at constant pressure).

4. Thermochemistry an exothermic process at constant pressure ∆H < 0.
an endothermic process at constant pressure ∆H > 0.

5. Standard state
The standard state of a substance at a specified temperature is its pure form at 1 bar.
standard state of liquid ethanol at 298 K is pure liquid ethanol at 298 K and 1 bar;
the standard state of solid iron at 500 K is pure iron at 500 K and 1 bar.
The standard enthalpy change for a reaction or a physical process is the difference between the products in their standard states and the reactants in their standard states, all at the same specified temperature.

6. Enthalpies of physical change
The standard enthalpy change that accompanies a change of physical state is called the standard enthalpy of transition and is denoted ∆trsH .
The standard enthalpy of vaporization,∆vapH .
The standard enthalpy of fusion, ∆fusH .

7. Exercise 2.16b
A certain liquid has ∆vapH = 32.0 kJ mol−1. Calculate q, w, ∆H, and ∆U when 0.75 mol is vaporized at 260 K and 765 Torr.

9. Enthalpies of physical change
Because enthalpy is a state function, a change in enthalpy is independent of the path between the two states.
the conversion of a solid to a vapour either as occurring by sublimation or as occurring in two steps, first fusion (melting) and then vaporization of the resulting liquid.

10. Enthalpies of physical change
The standard enthalpy changes of a forward process and its reverse differ in sign.

12. Enthalpies of chemical change

13. Standard enthalpy of combustion, ∆cHo
standard enthalpy of combustion, ∆cHo, is the standard reaction enthalpy for the complete oxidation of an organic compound to CO2 gas and liquid H2O.

14. Standard enthalpy of combustion, ∆cHo

15. Hess’s law
The standard enthalpy of an overall reaction is the sum of the standard enthalpies of the individual reactions into which a reaction may be divided.

16. Example 2.5 Using Hess’s law
                                                         
Example 2.5  Using Hess’s law
The standard reaction enthalpy for the hydrogenation of propene is −124 kJ mol−1.
The standard reaction enthalpy for the combustion of propane is −2220 kJ mol−1.
Calculate the standard enthalpy of combustion of propene.

18. Self Test 2.6
Calculate the enthalpy of hydrogenation of benzene from its enthalpy of combustion and the enthalpy of combustion of cyclohexane.

19. Standard enthalpy of formation ∆fHo
Standard enthalpy of formation, ∆fHo, of a substance is the standard reaction enthalpy for the formation of the compound from its elements in their reference states.
The standard enthalpies of formation of elements in their reference states are zero at all temperatures
the hydrogen ion in solution has zero standard enthalpy of formation at all temperatures

21. Standard enthalpy of formation ∆fHo

22. Illustration 2.7 Using standard enthalpies of formation
Calculate The standard reaction enthalpy of 2 HN3(l) + 2 NO(g) → H2O2(l) + 4 N2(g)

23. Exercise 2.17b 
The standard enthalpy of formation of phenol (C6H5OH) is −165.0 kJ mol−1. Calculate its standard enthalpy of combustion.

24. Exercise 2.18a 
The standard enthalpy of combustion of cyclopropane is −2091 kJ mol−1 at 25°C. From this information and enthalpy of formation data for CO2(g) and H2O(g), (a) calculate the enthalpy of formation of cyclopropane. (b) The enthalpy of formation of propene is kJ mol−1. Calculate the enthalpy of isomerization of cyclopropane to propene.

25. Exercise 2.18a  
From the following data, determine ∆fH for diborane,B2H6(g), at 298 K:

26. The temperature-dependence of reaction enthalpies Kirchhoff’s law

27. Example 2.6 Using Kirchhoff’s law
The standard enthalpy of formation of gaseous H2O at 298 K is − kJ mol−1. Estimate its value at 100°C given the following values of the molar heat capacities at constant pressure: H2O(g): J K−1 mol−1; H2(g): J K−1 mol−1; O2(g): J K−1 mol−1. Assume that the heat capacities are independent of temperature.

28. Estimate the standard enthalpy of formation of cyclohexene at 400 K.