CHEM 1050 Lecture Notes - Lecture 12: Joule

• School: University of Guelph
• Department: Chemistry
• Course: CHEM 1050
• Professor: Mario Monteiro

Document Summary

You were given 3 equations with corresponding h values. Need c2h2 on the product side so turn first equation around and change sign of h; Also you need two moles of c(s) so multiply the second equation and its h by. On monday we discovered that when g = 0 the reaction is at equilibrium. When g is negative the reaction is spontaneous as written. When g is positive a + b c or reaction is non spontaneous as written. If entropy (s) were not in this equation then all exothermic reactions ( h is negative) would have negative g (spontaneous) S contribution is ( - t s) and may increase or decrease tendency of reaction. When s is positive (more random final state) then - t s will have a negative contribution to g and will therefore increase tendency for reaction to be non- spontaneous.