Problem 11PE
Calculating an Enthalpy of Reaction from Enthalpies of Formation
(a) Calculate the standard enthalpy change for the combustion of 1 mol of benzene, C6H6(l), to CO2(g) and H2O(l).
(b) Compare the quantity of heat produced by combustion of 1.00 g propane with that produced by 1.00 g benzene
Use Table to calculate the enthalpy change for the combustion of 1 mol of ethanol:
C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l)
Table Standard Enthalpies of Formation,ΔHf°, at 298K
Chapter 12 Lecture Notes Things to remember o Remember that properties of gases can be related by PV=nRT (ideal gas law) o Remember that molecules of gases are far apart, while molecules in liquid and solid are closely packed o Remember that molecules can have polar bonds, due to differences in electronegativity of bonded atoms o Intramolecular bonds are strong Covalent: 100-400 kJ/mol Ionic: 700 -1100 kJ/mol o Intramolecular forces: forces holding atoms together to form molecules (covalent bonds, ionic bonds) o Intermolecular forces: electrostatic interactions between molecules that are weaker than forces between oppos
