My past report about thermochemistry. It includes the application of thermochemistry, the meaning of calorimetry, the application of Hess Law, and enthalpy.

1. THERMOCHEMICAL EQUATION
CALORIMETRY
HESS’ LAW
THERMO
CHEMISTRYANJ CASTILLO // ST. AGATHA

5. HEATS OF FORMATION,
Hf, represents an equation in which one
mole of product is made from elements.
4 Al (s) + 3 O2 (g) -> 2 Al2O3 (s) q = -3400 kJ

6. The equation shows the formation of
aluminum oxide from the pure elements. Re-
write it such that only one mole of
aluminum oxide is produced.
4 Al (s) + 3 O2 (g) -> 2 Al2O3 (s) q = -3400 kJ_ __ __
2 2 2
2 Al (s) + 3/2 O2 (g) -> Al2O3 (s) q = -3400 kJ

7. Calculate the het of this new reaction and
restart is ass enthalpy, the energy
absorbed/released per mole of reaction.
2 Al (s) + 3/2 O2 (g) -> Al2O3 (s) q = -3400 kJ
4 Al (s) + 3 O2 (g) -> 2 Al2O3 (s) q = -3400 kJ
Hf = -1700

15. Determine H 25 C for the reaction:
2 FeO2 (g) + ½ O2 -> Fe2O3 (S)
Fe (s) + ½ O2 (g) -> FeO H 25 C = -272.0 kJ
2 Fe (s) + 3/2 O2 (g) -> Fe2O3 H 25 C = -825 kJ

16. Eq. 1
Eq. 2
Eq. (1)’: 2 FeO (s) -> 2 Fe + O2 (g)
H 25 C = -[2(-272.0 kJ)] = 544 kJ

17. THANK
YOU