2. 1 Hesss Law Start Finish A State Function: Path independent. Both lines accomplished the same result, they went from start to finish. Net result = same.

3. 2 Determine the heat of reaction for the reaction: 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) Using the following sets of reactions: N 2 (g) + O 2 (g) 2NO(g) H = 180.6 kJ N 2 (g) + 3H 2 (g) 2NH 3 (g) H = - 91.8 kJ 2H 2 (g) + O 2 (g) 2H 2 O(g) H = -483.7 kJ Hint: The three reactions must be algebraically manipulated to sum up to the desired reaction. and.. the H values must be treated accordingly.

4. 3 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) Using the following sets of reactions: N 2 (g) + O 2 (g) 2NO(g) H = 180.6 kJ N 2 (g) + 3H 2 (g) 2NH 3 (g) H = - 91.8 kJ 2H 2 (g) + O 2 (g) 2H 2 O(g) H = -483.7 kJ Goal: NH 3 : O2 O2 : NO: H 2 O: Reverse and x 2 4NH 3 2N 2 + 6H 2 H = + 183.6 kJ Found in more than one place, SKIP IT (its hard). x2 2N 2 + 2O 2 4NO H = 361.2 kJ x3 6H 2 + 3O 2 6H 2 O H = -1451.1 kJ

5. 4 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) Goal: NH 3 : O 2 : NO: H 2 O: Reverse and x2 4NH 3 2N 2 + 6H 2 H = + 183.6 kJ Found in more than one place, SKIP IT. x2 2N 2 + 2O 2 4NO H = 361.2 kJ x3 6H 2 + 3O 2 6H 2 O H = -1451.1 kJ Cancel terms and take sum. 4NH 3 + 5O 2 4NO + 6H 2 O H = - 906.3 kJ Is the reaction endothermic or exothermic?

6. 5 Determine the heat of reaction for the reaction: C 2 H 4 (g) + H 2 (g) C 2 H 6 (g) Use the following reactions: C 2 H 4 (g) + 3O 2 (g) 2CO 2 (g) + 2H 2 O(l) H = -1401 kJ C 2 H 6 (g) + 7/2O 2 (g) 2CO 2 (g) + 3H 2 O(l) H = -1550 kJ H 2 (g) + 1/2O 2 (g) H 2 O(l) H = -286 kJ Consult your neighbor if necessary.

7. 6 Determine the heat of reaction for the reaction: Goal: C 2 H 4 (g) + H 2 (g) C 2 H 6 (g) H = ? Use the following reactions: C 2 H 4 (g) + 3O 2 (g) 2CO 2 (g) + 2H 2 O(l) H = -1401 kJ C 2 H 6 (g) + 7/2O 2 (g) 2CO 2 (g) + 3H 2 O(l) H = -1550 kJ H 2 (g) + 1/2O 2 (g) H 2 O(l) H = -286 kJ C 2 H 4 (g) :use 1 as is C 2 H 4 (g) + 3O 2 (g) 2CO 2 (g) + 2H 2 O(l) H = -1401 kJ H 2 (g) :# 3 as is H 2 (g) + 1/2O 2 (g) H 2 O(l) H = -286 kJ C 2 H 6 (g) : rev #2 2CO 2 (g) + 3H 2 O(l) C 2 H 6 (g) + 7/2O 2 (g) H = +1550 kJ C 2 H 4 (g) + H 2 (g) C 2 H 6 (g) H = -137 kJ

8. 7 Summary: enthalpy is a state function and is path independent.

9. 8

10. 9 Standard Enthalpies of formation:

11. 10 Thermodynamic Quantities of Selected Substances @ 298.15 K