CHEM 1E03 Lecture Notes - Lecture 25: Calorimetry, Sulfur Trioxide, Joule

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1E03
• Professor: Randall Dumont; Linda Davis

Document Summary

Calorimetry and enthalpy change: h = h1 + h2 = -c t, h: enthalpy change: change from conversion of reactants to products, c: heat capacity, t: change in temperature (kelvins, note: all variables must be for the same entity. Additional notes: h depends on the amount of reactant converted into product (proportional, the enthalpy of reaction = change in enthalpy per mol of extent of reaction. N = cv: h reaction = h / n, = -1. 12 / 0. 02, = -56 kj / mol. Exothermic: freezing, condensation, deposition, bond formation, breaking of weaker bonds to form stronger ones. Hess"s law: the enthalpy of a reaction, is the sum of the enthalpies, h = h final h initial, h = h forward + h reverse = 0, h reverse = -( h) forward. Note: sign is reversed for forward: this applies for any reaction with the same initial reactants and final product states.