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Published byJoseph Willis Modified over 9 years ago
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Chemical Equilibrium Click here for blue bottle demonstration
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Click here for a tutorial
Chemical Equilibrium 2NO2 ⇄ N2O4 These reactions can be reversible. Click here for a tutorial [
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Le Chatelier’s Principle
If a change in conditions occurs, the equilibrium position will shift to cancel out the change. Click here for a tutorial
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Le Chatelier’s Principle
Changing Concentration Equilibrium shifts away from the excess concentration [
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Hemoglobin, Blood, & Oxygen
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Le Chatelier’s Principle
Example: NH4Cl ⇄ NH3 + HCl If more acid (HCl) is added, which side will be “favored”? Reactants!
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Le Chatelier’s Principle
Changing Pressure (gases only) If pressure increases, reaction changes to side with fewer moles. [
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The opposite is also true…
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Le Chatelier’s Principle
Example: CH4 (g) + 2 O2 (g) ⇄ CO2 (g) + 2 H2O (l) If the pressure is increased, which side would be “favored”? Products! (3 moles gas : 1 mole gas)
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Le Chatelier’s Principle
Changing Temperature If temperature increases, reaction goes to endothermic side. [
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Le Chatelier’s Principle
Click here for Nitrogen Monoxide video. Clip 1: 2 NO2 (g) ⇄ N2O4 (g) + energy (Brown Gas) (White Solid) Clip 2: NO2 (g) + NO (g) ⇄ N2O3 (g) + energy (Brown Gas) (Blue Solid)
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