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Understanding Le Châtelier’s Principle: Equilibrium Shifts in Chemical Reactions

Le Châtelier’s Principle states that if an external change is imposed on a system at equilibrium, the system will adjust to counteract that change, re-establishing equilibrium. Factors influencing this include concentration, temperature, and pressure. For instance, adding a reactant shifts the reaction away from that component, while temperature changes can alter the equilibrium constant (K). This principle helps predict responses to changes such as increased pressure or temperature, guiding reactions toward the formation of products or reactants.

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Understanding Le Châtelier’s Principle: Equilibrium Shifts in Chemical Reactions

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  1. LeChatlier’s Principle

  2. Le Châtelier’s Principle • . . . if a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change.

  3. Effects of Changes on the System • 1.Concentration: The system will shift away from the added component. • 2. Temperature: K will change depending upon the temperature .

  4. Effects of Changes on the System (continued) • 3. Pressure: • a. Addition of inert gas does not affectthe equilibrium position. • b.Decreasing the volume shifts the equilibrium toward the side with fewer moles of gases.

  5. Predict the “shift” for each type of disturbance to the equilibrium 2NOBr(g) 2NO(g) + Br2(g) Kp=0.16 at 25°C ΔH = +16.3kJ • Adding more Br2(g) • Removing some NOBr(g) • Decreasing the temperature • Increasing the container volume

  6. 2NO2 (g) ↔ N2O4 (g) ΔH = -58.0 kJPredict the effect of each of the following changes on this system atequilibrium (drive forward reaction, drive reverse reaction, no effect).a) add N2O4b) remove NO2c) increase the volume d) decrease the temperaturee) Add N2

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