Lecture 14 - Chapter 6 Reactivity & Mechanisms - Edubirdie

University:
York University
Course:
CHEM 1000 | Chemical Structure
Academic year:

2021
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87

Pages:

2
Author:

Niklas

Lecture 14 (02/25/21) Chem. Reactivity & Mechanisms ΔG° = ΔH° - TΔS° ΔH < 0 ΔH > 0 ΔS > 0 Spontaneous Spontaneous at all T at high T ΔG < 0 ΔG > 0 ΔS < 0 Spontaneous Non-spontaneous at low T at all T TAS Small Rate Rate = Ae^(-Ea/RT) Arrhenius Eq. (Rates) Equilibrium ΔG° = -RTlnK Case 1 Rate difference C + D are formed faster C + D are less thermodynamically stable (in this case) Free Energy (G) Reaction Coordinate A + B → C + D → E + F Formed Faster than E/F Kinetic Products 1. Low temp, Short rxn time → Kinetic Prod. 2. High temp, Long rxn time → Thermodynamic Prod.

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