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Equilibrium

Equilibrium refers to the point where the rate of the forward and reverse reactions are equal. This helpful guide explains how concentration, pressure, and temperature can shift an equilibrium reaction. Test your knowledge with an example reaction!

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Equilibrium

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  1. Equilibrium • Equilibrium is when the rate of forward is the same as reverse; • this refers to speed of the reaction; concentration will remain unchanged, • this does not mean the concentration is equal or must have the same value for each side.

  2. Equilibrium! Only the following will shift a reaction at equilibrium: 1. Change in concentration: If you add more reactant = make more product (R) If you add more product = make more reactant (L)

  3. Remove reactant/remove product Remove reactant = replaces reactant (L) Remove product = replaces product (R)

  4. 3. Change in pressure (must all be gases in equation) Increase pressure = less space = shift to side with smallest amount of moles Decrease pressure = more space = shift to side with greatest amount of moles

  5. Do not be fooled! Change in volume is just another way to say change in pressure!

  6. Change in temperature. Exothermic = heat is a product; heat is released Endothermic = heat is a reactant; heat is absorbed

  7. Test Yourself! 4NH3(g) + 5O2(g)  4NO(g) + 6H2O(g) + heat Which way will the equilibrium shift for the above reaction? • Increase concentration of oxygen • Increase the pressure • Increase the temperature • Remove NO

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