1. Le Chatelier's Principle

2. What if the conditions of the equilibrium changed? Le Chatelier’s principle states that if a closed system at equilibrium is subjected to a change(stress), things will happen to counteract that change (regain back balance).

3. The effect of Temperature changes Temperature affects heat terms in a reaction. If you increase temperature, you are increasing the heat term(energy). Therefore, the reaction will shift to use up this “extra” heat/energy and go back to original state.

4. The Effect of Temperature Changes A + B ⇌ C + Energy Change: increase Tempreaction- shifts left

5. The Effect of Temperature Changes A + B + Energy ⇌ C Change: increase Tempreaction- shifts right

6. The Effect of Temperature Changes A + B + Energy ⇌ C Change: decrease Tempreaction- shifts left

7. The Effect of Concentration Changes

8. Adding a reactant or product shifts the reaction in the direction that removes them/uses them up. A + B ⇌ C + Energy reaction- shifts rightchange- increase [A]

9. Adding a reactant or product shifts in the direction that removes them. A + B ⇌ C + Energy stress- increase [C]reaction- shifts left

10. Removing a reactant or product shifts reaction to make MORE. A + B ⇌ C + Energy change- decrease [A]reaction- shifts left

11. Removing a reactant or product shifts reaction to make more. A + B ⇌ C + Energy change- decrease [C]reaction- shifts right

12. Effect of pressure changes

13. A (g) +B (g) ⇄ AB (g) 2 mols 1 mol more pressureless pressure Usually we refer only to gases (g) when we talk about pressure changes. Those pressure changes we control by changing the volume.

14. As you know… If you decrease the volume, you increase the pressure. If you increase the volume, you decrease the pressure. Also, increasing pressure increases the concentrations of ALL gaseous species found.

15. Where to start? First identify where there is more pressure or where there is less pressure by counting up the molecules of gas you have on each side.

16. 4HCl (g) + 2O 2(g) ⇄ 2H 2 O (l) + 2Cl 2(g) If we decreased the volume, pressure will ________ and so the reaction will go to low pressure side. less pressure 6 mols2 mols more pressure

17. 2SO 3(g) ⇄ 2SO 2(g) + O 2(g) more pressure less pressure 2 gas 3 gas If we increased the volume, pressure will _________, so the reaction responds by… increasing pressure again and goes to more pressure side

18. We decrease the volume, we increase pressure! Increasing the pressure by decreasing the volume shifts to the eqlm fewest gas molecules. Only (g) count for gas particles. 4HCl (g) + 2O 2 (g) ⇄ 2H 2 O (l) + 2Cl 2 (g) + 98kJ The reaction responds by shifting to right to decrease the pressure! 6262 All concentrations go up!

19. 5A (g) + 2B (g) ⇌ 4C (g) + 5D (g) We ⇑ P The Reaction opposes and goes to low pressure side ⇓ P 7979 We ⇓ V Shifts left

20. 4A (g) + 2B (g) ⇌ 3C (g) + 2D (g) 6565 We ⇓ V We ⇑ P What volume change shifts right?

21. 2A (g) + 2B (g) ⇌ 3C (g) + 4D (g) We ⇓ P 4747 We ⇑ V What volume change shifts right?

22. 4HCl (g) + 2O 2 (g) ⇄ 2H 2 O (l) + 2Cl 2 (g) + 98kJ Describe the shift in the above equilibrium system for each stress indicated. StressShift[HCl][O 2 ][Cl 2 ] ↓ ← ↑ V ↑↑ ↑←↑ [Cl 2 ] ――――Add water ↓↓ ↑ ← ↑↑↓→ ↑ [HCl] ↓ [O 2 ] ↓ ↓ When the volume increases, pressure decreases and all concentration go down

23. reactants Adding a catalyst does not shift the equilibrium Equilibrium is attained faster Forward and reverse rates are increased by the same amount products

24. Adding an inert (non-reactive) gas does not shift the equilibrium. Adding Ne (g) 2NH 3(g) ⇌ N 2(g) + 3H 2(g) No shift!

25. Homework Exercises 17-23 on page 54. Exercises 24-26, do NOT graph, only state what each change/stress would do to the equilibrium (ie; where it shifts it)