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Catalyst

Take out your HW!. Catalyst. Objectives I can define Le Chatelier’s principle. I can describe factors that shift chemical equilibrium. Agenda Catalyst Exit Slip Review Simulation: Shifting Equilibrium Le Chatelier’s Principle.

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Catalyst

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  1. Take out your HW! Catalyst • Objectives • I can define Le Chatelier’s principle. • I can describe factors that shift chemical equilibrium. • Agenda • Catalyst • Exit Slip Review • Simulation: Shifting Equilibrium • LeChatelier’s Principle Make a list of everyday adjustments that are made to relieve stress on a system or stabilize a system. Example: If we are hungry, we eat to get the energy we need.

  2. Exit Slip Review • Assignment: Write at least 5 sentences explaining what chemical equilibrium is. Use examples from class. Use the key terms: reversible reaction, completion reaction, and chemical equilibrium. • Sample Answer: Chemical equilibrium is a state of balance in which the rate of a forward reaction equals the rate of the reverse reaction. At equilibrium, the concentrations of the reactants and products stop changing. However, the amount of reactant and product may not be equal. Chemical equilibrium involves reversible reactions that proceed in both the forward and reverse direction. A completion reaction does not go to equilibrium because all of the reactants turn into products. This is called going to “completion”. In the bucket equilibrium demonstration, the system ended up at equilibrium because the amount of water transferred either way became the same.

  3. Exit Slip Review Continued • This student paragraph received a 4: A chemical equilibrium is when a chemical or substance equals out or moves at the same rate. A reversible reaction is when the products and reactants can switch or reverse the opposite way. A completion reaction is when they only move forward. When they move at the same rate it will reach a equilibrium. For example, in the water demonstration, one started out with a lot of water and the other didn’t. Since they were moving at the same rate, they reached equilibrium.

  4. 9b Make Up Assignment • pp. 522 #20 – Answer and justify your answer. • Correct and then write a final draft of your chemical equilibrium paragraph.

  5. Computer Simulation: Equilibrium • Continue on your notes from “Day 3”. • Answer the questions on your worksheet as we go.

  6. What is Le Chatelier’s Principle? • For a reversible process at equilibrium, when conditions of concentration, temperature, or pressure are changed, the reaction shifts in a direction that will counteract the stress and restore equilibrium.

  7. Think Box: In my own words. • Rewrite Le Chatelier’s Principle in your own words. • You will have 2 minutes to write on your own. • You will have 2 minutes to discuss with the person next to you and revise your work.

  8. How does Le Chatelier’s Principle work? Example #1: N2(g) + 3H2(g) ↔ 2NH3(g) + heat Left / reverse To remove the extra heat Right/ forward To replace the lost heat Right/ forward To decrease the extra reactant Left / reverse To decrease the extra product Right/ forward To decrease the moles of gas Left / reverse To increase the moles of gas

  9. Example #2: N2O4(g) + heat ↔ 2NO2(g) Right/ forward To remove the extra heat Left / reverse To replace the lost heat Right/ forward To decrease the extra reactant Left / reverse To decrease the extra product Left / reverse To decrease the moles of gas Right/ forward To increase the moles of gas

  10. White Board Practice • Instructions: • Write your answer on your white board. • When Ms. Boon says go, hold up your white board.

  11. White Board Practice • PCl5 PCl3 + Cl2 • In order to shift the equilibrium to the right, the rate of the _____________________________ reaction will increase. • In order to shift the equilibrium to the left, the rate of the ___________________________ will increase.

  12. White Board Practice • PCl5 PCl3 + Cl2 • Adding more product shifts the equilibrium to the ___________. • Adding more product increases the rate of the ______________________________ reaction. • Taking away some of reactant shifts the equilibrium to the _________________.

  13. White Board Practice • 2 H2(g) + O2(g) ↔2 H2O (g) • Taking away some H2 will increase the rate of the _______________ reaction. • Decreasing the pressure will shift the equilibrium to the ________.

  14. White Board Practice • 6CO2 + 6H2O + 12 kJ  C6H12O6 + 6CO2 • Increasing the temperature will increase the rate of the __________________ reaction. • Increasing the temperature shifts the equilibrium to the ____________________.

  15. Independent Practice • Expectations: • You make work with the person next to you. • You will use respectful academic language and speak at a noise level at which only people next to or across from you can hear. • Tools: • You may use all your notes and worksheets. • What do I when I am done? • Raise your hand to get a stamp. Then check your answers. • Homework: • HW: pp. 518 #2, 3, 9; pp. 522 #18 &19

  16. Exit Slip • Part 1: • Write at least 5 sentences explaining what chemical equilibrium is. Use examples from class. Use the key terms: reversible reaction, completion reaction, and chemical equilibrium. • Part 2: • Grade your level of understanding of the current unit on a scale of 1 – 4. 4 is the highest. • Homework: • HW: pp. 518 #2, 3, 9; pp. 522 #18 &19

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