From: Andrew Lorimer <andrew@lorimer.id.au>
Date: Thu, 14 Mar 2019 06:58:29 +0000 (+1100)
Subject: [chem] activation energy, kinetic energy, catalysts
X-Git-Tag: yr12~207
X-Git-Url: https://git.lorimer.id.au/notes.git/diff_plain/3ab8faeb27f00c045f8e307b27d1ff3c17cf7307

[chem] activation energy, kinetic energy, catalysts
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+# Rates and Equilibria
+
+## Energy profile diagrams
+
+$$E_A = E_{\text{max}} - E_{\text{initial}}$$
+
+- Energy always needed to initiate reaction (break bonds of reactants)
+- Reactant particles must collide at correct angle, energy etc
+- Most collisions are not fruitful
+
+![](graphics/endothermic-profile.png)
+![](graphics/exothermic-profile.png)
+
+**Ways to increase rate of reaction:**
+
+1. Increase surface area
+2. Increase concentration/pressure
+3. Increase temperature
+
+## Kinetic energy
+
+Temperature - measure of _avg_ kinetic energy of particles. Over time each particle will eventually have enough energy to overcome $E_A$.  
+Note same distribution indicates same temperature.  
+![](graphics/ke-temperature.png)
+
+## Catalysts
+
+- alternate reaction pathway, with lower $E_A$
+- increased rate of reaction
+- involved in reaction but regenerated at end
+
+**Homogenous** catalyst: same state as reactants and products, e.g. Cl* radicals.  
+**Hetrogenous** catalyst: different state, easily separated. Preferred for manufacturing.
+![](graphics/catalyst-graph.png)