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Le Chatelier's Principle

Le Chatelier's Principle. If a system at equilibrium is altered in a way that disrupts the equilibrium, the system will adjust in such a way as to counter the change. N 2(g) + 3 H 2(g) ⇆ 2 NH 3(g) + energy. Rates of Reaction for Reversible Reactions. FACTORS AFFECTING EQUILIBRIUM.

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Le Chatelier's Principle

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  1. Le Chatelier's Principle If a system at equilibrium is altered in a way that disrupts the equilibrium, the system will adjust in such a way as to counter the change. N2(g) + 3 H2(g)⇆ 2 NH3(g) + energy

  2. Rates of Reaction for Reversible Reactions

  3. FACTORS AFFECTING EQUILIBRIUM • CONCENTRATION • TEMPERATURE • PRESSURE

  4. 1. CONCENTRATION CONCENTRATION CHANGES FAVORING FORWARD REACTION: • Addition of more reactants; • Removal of some products

  5. Effect of Increased Concentration on Equilibrium

  6. Effect of Decreased Concentration on Equilibrium

  7. N2(g) + 3 H2(g)⇆ 2 NH3(g) + energy Addition of N2 or H2 or removal of NH3 would result to an increase in NH3.  Removal of N2 or H2 or addition of NH3 would result to an increase in N2 and H2. 

  8. TEMPERATURE • Increasing temperature favors the forward reaction of endothermic reactions • Increasing temperature favors the backward reaction of an exothermic reactions

  9. N2(g) + 3 H2(g)⇆ 2 NH3(g) + energy exothermic Lowering of temperature would result to an increase in NH3.  Increasing temperature would result to an decrease in NH3. 

  10. PRESSURE - Increasing pressure favors the direction of reaction which will produce lesser number of particles.

  11. N2(g) + 3 H2(g)⇆2 NH3(g) + energy There are 4 moles of the reactant and 2 moles of the product. Increasing pressure favors the formation of lesser number of moles therefore producing moreNH3 and using up N2 and H2. 

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