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LE CHATELIER PRINCIPLE: Understanding how equilibrium responds to changes
- 1. LE CHATELIER'S PRINCIPLE UNDERSTANDINGHOW EQUILIBRIA RESPOND TO CHANGES
- 2. CONTENT • Introduction toLe Chatelier's Principle • Effect of Temperature • Effect of Pressure • Effect of Concentration (No. of Molecules) • Effect of Catalyst • Summary
- 3. INTRODUCTION TO LECHATELIER'S PRINCIPLE Definition: When a system at equilibrium is disturbed by a change in temperature, pressure, or concentration, the system shifts its equilibrium position to counteract the disturbance.
- 4. EFFECT OF TEMPERATURE Principle: •Increasing temperature favors the endothermic reaction. • Decreasing temperature favors the exothermic reaction. Example: • N (g) + 3H (g) 2NH (g) + heat ₂ ₂ ⇌ ₃ • Increase in temperature → shifts left • Decrease in temperature → shifts right
- 5. EFFECT OF PRESSURE Principle: •Increase in pressure → side with fewer gas molecules • Decrease in pressure → side with more gas molecules Example: • N (g) + 3H (g) 2NH (g) ₂ ₂ ⇌ ₃ • 4 moles → 2 moles • Increase in pressure → shifts right
- 6. EFFECT OF CONCENTRATION(NO. OF MOLECULES) Principle: • Adding reactants → shifts right • Removing products → shifts right Example: • CH COOH CH COO + H ₃ ⇌ ₃ ⁻ ⁺ • Add CH COOH → shifts right ₃ • Remove H → shifts right ⁺
- 7. EFFECT OF CATALYST Principle: •Catalyst does not affect equilibrium position • It only speeds up the rate of reaching equilibrium Example: • Haber process (Fe catalyst): • N + 3H 2NH ₂ ₂ ⇌ ₃ • Catalyst speeds up NH production but yield remains same ₃
- 8. SUMMARY Factor Direction ofShift Affected By Temperature Depends on exo/endo Yes Pressure Toward fewer gas molecules Yes (gases) Concentration Toward the opposite side Yes Catalyst No shift No
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