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CHEMICAL EQUILIBRIUM Chapter 16

CHEMICAL EQUILIBRIUM Chapter 16. OBJECTIVE. Distinguish between reversible and completion reactions Understand Equilibrium Define/ apply the terms system and stress to reversible reactions Le Chatlier’s Principle. Reversible Reactions. H 2 + I 2 ↔ 2HI

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CHEMICAL EQUILIBRIUM Chapter 16

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  1. CHEMICAL EQUILIBRIUMChapter 16

  2. OBJECTIVE • Distinguish between reversible and completion reactions • Understand Equilibrium • Define/ apply the terms system and stress to reversible reactions • Le Chatlier’s Principle

  3. Reversible Reactions H2 + I2 ↔ 2HI • the products may react back to original reactants. • “closed system”: ONLY if all reactant are present • If one piece is completely gone it has ”gone to competition” and no longer reversible

  4. TWO REACTIONS • only difference is the Direction H2 + I2↔ 2HI reactants products 2HI ↔ H2 + I2 Left Right

  5. Examples: Reversible Reactions. • Unopened Soda • Breathing • Rechargeable batteries • Color changing shirt

  6. Equilibrium • The state in which a chemical reaction and its reverse reaction occur at the same rate.

  7. Equilibrium = No change in amount over time

  8. Equilibrium achieved Reversible Reactions Product conc. increases and then becomes constant at equilibrium Reactant conc. declines and then becomes constant at equilibrium

  9. “System” • Any reversible reaction H2 + I2↔ 2HI noted by the double arrow; ↔

  10. “stressing a system” • Pick reversible reactions that have different colored products. • EXAMPLES T –shirt ball • Stress: done to change the ratio color change means change ratio of two products

  11. Le Chatelier’s Principle • If a system at equilibrium is stressed, it will react to undo the stress.

  12. Le Chatelier’s Principle • Anything YOUdo(stress) to a reversible reaction, the systemreacts in a way to UNDO that change • Remember there are TWO reactions going in every reversible reaction.

  13. Shifting Equilibrium • Change Temperature • Change concentration of Cl- CuCl4(aq)↔ Cu+(aq)+ Cl-(aq)+ heat Left: GREEN Right BLUE • Add Temperature or Cl- : Green/ right • Remove heat or Cl: Blue / Left

  14. Temperature ADD energy or REMOVE energy Will cause opposite results Science is fun 29778 bleaching

  15. Concentration:Amount ADD reactant or REMOVE reactant Will cause opposite results Science is fun 31918 Cu and hydrogen

  16. Pressure Used for gases Easiest way to measure the amount of a gas Same affect as changing the concentration

  17. Equilibrium Disk 6C32 Pink to blue Co(H2O)6Cl2---> Co(H2O)4Cl2 + 2 H2O Equilibrium systems are • DYNAMIC (in constant motion) • REVERSIBLE • can be approached from either direction Blue to pink Co(H2O)4Cl2+ 2 H2O ---> Co(H2O)6Cl2

  18. Le Chatelier’s Principle • If youADDreactants , The system will REMOVEreactants by making more products. • If youREMOVEreactants , The system will ADDreactants by USING (reacting) products.

  19. LEFT: RIGHT: ↔

  20. L R L L R L L R R R

  21. STRESS to SYSTEM Three stress’s are • Temperature • Concentration • Pressure.

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