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Le Chatelier’s Principle

Le Chatelier’s Principle. Henry Louis Le Chatelier. Born on Oct. 8, 1850 Between the years 1884-1914 he published about 30 papers on either the principle of chemical equilibrium or the variation of the solubility of salts in an ideal solution.

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Le Chatelier’s Principle

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  1. Le Chatelier’s Principle

  2. Henry Louis Le Chatelier • Born on Oct. 8, 1850 • Between the years 1884-1914 he published about 30 papers on either the principle of chemical equilibrium or the variation of the solubility of salts in an ideal solution. • He taught chemistry at the Collège de France, from 1898 – 1907.

  3. Le Chatelier’s Principle • This principle is used to describe the effect a change in conditions can have on a chemical equilibrium. • “If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change.” (Le Chatelier)

  4. How to use the principle (concentration) • An increase in the concentration of the reactants, means a shift to the right. (makes more products) • An increase in the concentration of the products, means a shift to the left. (makes more reactants) • If there is a decrease then the shift is to the opposite side. • ex. CO + 2 H2 ⇌ CH3OH

  5. How to use the principle(temperature) • An increase in temperature causes the equilibrium position of a reaction to shift in the direction that absorbs heat. Hint: Treat heat like a reactant or product. • ex. N2 + 3 H2 ⇌ 2 NH3 + 92kJ

  6. How to use the principle (pressure) • An increase to the pressure results in a shift towards the side with the least moles of gas. • A decrease in the pressure results in a shift towards the side with the most moles of gas. • ex. N2(g) + 3 H2(g) ⇌ 2 NH3(g)

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