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Equilibrium

Equilibrium. Equilibrium. Equilibrium: When the rate of the forward reaction equals the rate of the reverse reaction and the amount of the reactants and products remain unchanged. Equilibrium. Demo Beaker 1 is the reactants Beaker 2 is the products

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Equilibrium

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  1. Equilibrium

  2. Equilibrium Equilibrium: When the rate of the forward reaction equals the rate of the reverse reaction and the amount of the reactants and products remain unchanged.

  3. Equilibrium • Demo • Beaker 1 is the reactants • Beaker 2 is the products • The little beaker are the rates that the reverse reactions are occurring at At the beginning are the rates the same? One the rates are the same what happens to the amount of products and reactants?

  4. Le Châtelier’s Principle If a system at equilibrium is subject to a stress, the equilibrium is shifted in the direction to relieve the stress. Stress can be: • A change in the amounts of products or reactants • A change in the volume of the container • A temperature change

  5. Le Châtelier’s Principle If a system at equilibrium is subject to a stress, the equilibrium is shifted in the direction to relieve the stress. Imagine reversible equation like a teeter-totter if the equation is at equilibrium the teeter-totter is balanced Reactants Products

  6. Le Châtelier’s Principle Let say I added more products to the container. Now my teeter-totter is off balanced. Think back to when you were on a teeter-totter last, what did you do if some one weight more then the other? Reactants Products Reactants ← Products

  7. Le Châtelier’s Principle 3H2(g) + N2(g) ↔ 2NH3(g) So let say we have the given reaction at equilibrium. So the it’s happy and balanced. What if I added some hydrogen gas? How would the reaction have to shift to fix the equilibrium? 3H2 + N2 2NH3

  8. Le Châtelier’s Principle What if I added some hydrogen gas? How would the reaction have to shift to fix the equilibrium? The teeter-totter would tilt left and you would have to shift right to fix it. Shift Right 2NH3 3H2 + N2

  9. Le Châtelier’s Principle 3H2(g) + N2(g) ↔ 2NH3(g) Now let say I removed some nitrogen gas, what happens to the teeter-totter? How do you fix it? Shift Left 3H2 + N2 2NH3

  10. Le Châtelier’s Principle 3H2(g) + N2(g) ↔ 2NH3(g) What if I changed the volume of the container? Volume only affects gases. You have to look at the moles of gas on each side of the reaction. This reaction has 4 moles of gas on the reactant side and 2 moles of gas on the product side.

  11. Le Châtelier’s Principle 3H2(g) + N2(g) ↔ 2NH3(g) If you make the container smaller the reaction always shift to the side with the least moles of gas. Shift Right If you make the container bigger it always shifts to the side with the most moles of gas. Shift Left

  12. Le Châtelier’s Principle If you know your reaction is endothermic that means the reaction absorbs heat and heat is a reactant Heat + 3H2(g) + N2(g) ↔ 2NH3(g) If you know your reaction is exothermic that means the reaction releases heat and heat is a product 3H2(g) + N2(g) ↔ 2NH3(g) + Heat

  13. Le Châtelier’s Principle If I told you the reaction was exothermic, what would happen if you cooled the reaction. 3H2(g) + N2(g) ↔ 2NH3(g) + Heat Shift right 2NH3 + Heat 3H2 + N2

  14. Practice 2SO3(g) ↔ 2SO2(g) + O2(g) How would the reacts shift if: • Oxygen gas was added? • The volume of the container increased? • Sulfur trioxide was removed? • Sulfur dioxide was removed? • The react was endothermic and was heated up? Shift Left Shift Right Shift Left Shift Right Shift Right

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