CHEM 1E03 Lecture Notes - Lecture 39: Lattice Energy, Jmol, Silver Chloride

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

Document Summary

2017 exam solutions were taken up this class: n gas should be larger than zero for there to be an increase of energy. Therefore, the answer is none: you have to assume that g and s are independent of temperature. Option (i) x2 g because you are forming to co from its elements. Use lattice enthalpy to determine that g1 g2 = -51-1/2(-274), therefore it is false. Option (ii) consists of both having negative g, therefore this statement is true. T s, so use s = ( h2 - g2) / t from rearranging. After substituting values the magnitude of the answer is correct, although it has the wrong sign (must be +). Option (iv) is under standard conditions, and g must be negative for the reaction to be spontaneous. Look at the g value provided in the question: h = products - reactants.