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Catalyst. Objectives I can define Le Chatelier’s principle. I can describe factors that shift chemical equilibrium. Agenda Catalyst Video Investigation: Equilibrium Le Chatelier’s Principle Exit Slip.

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Catalyst

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Catalyst

Catalyst

  • Objectives

  • I can define Le Chatelier’s principle.

  • I can describe factors that shift chemical equilibrium.

  • Agenda

    • Catalyst

    • Video Investigation: Equilibrium

    • LeChatelier’s Principle

    • Exit Slip

Pick up a whiteboard and marker and complete the following benchmark review question:

If each of these flasks has the same number of gas molecules inside, which one has the lowest pressure?

(a) Flask 1(c) Flask 2

(b) Flask 3(d) Flask 4


Video investigation dynamic equilibrium

Video Investigation: Dynamic Equilibrium

  • Answer the following questions on a white board:

  • What is dynamic equilibrium?

  • Explain the example of dynamic equilibrium in the video.

  • Can you come up with your own example?


What is le chatelier s principle

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.


Think box in my own words

Think Box: In my own words.

  • First, watch the video explain Le Chatelier’s Principle.

  • 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.

In an equilibrium system, when there is a change in conditions, the equilibrium will shift to counteract or undo the change.


Catalyst

  • add reactants or take away products causes shift to the right (forward)

  • add product or take away reactants causes shift to the left (reverse)

  • increase temp causes shift to endothermic side

  • decrease temp cause shift to exothermic side

  • increase pressure causes shift to less moles of gas

  • decrease pressure causes shift to more moles of gas


How does le chatelier s principle work

What will undo the change?

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


Catalyst

What will undo the change?

  • 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


Check for understanding

Check for Understanding

  • Compare the charts for example 1 and 2 in your notes. Why does increasing the temperature cause different shifts in equilibrium?

    • (1) The affect of changing temperature is random.

    • (2) The shift is to the left for endothermic reactions and to the right for exothermic reactions.

    • (3) The shift is to the right for endothermic reactions and to the left for exothermic reactions.


Check for understanding1

Check for Understanding

  • Compare the charts for example 1 and 2 in your notes. Why does increasing the pressure cause different shifts in equilibrium?

    • (1) The affect of changing pressure is random.

    • (2) The shift is to the side with less moles of gas to counteract the increase in pressure.

    • (3) The shift is to the side with more moles of gas to counteract the increase in pressure.


White board practice

White Board Practice

  • Instructions:

  • Write your answer on your white board.

  • When Ms. Boon says go, hold up your white board.


Answer the question as you watch the video

Answer the question as you watch the video…

  • List all reversible processes that you saw in the video. What caused the processes to continue or change directions?


White board practice1

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.


White board practice2

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 _________________.


White board practice3

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 ________.


White board practice4

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 ____________________.


Catalyst1

Catalyst

  • Objectives

  • I can define Le Chatelier’s principle.

  • I can describe factors that shift chemical equilibrium.

  • Agenda

    • Catalyst

    • Video Investigation: Equilibrium

    • LeChatelier’s Principle

    • Exit Slip

Find your folder and your returned Chemistry work.

Take about 4 minutes to organize your folder for student led conferences. Put the most recent items on the top.

Pass in your homework - The article questions.


Le chatelier s principle video demo

Le Chatelier’s Principle Video Demo

  • Answer the following questions on the back of your notes handout.

  • Copy the chemical reaction equation for the synthesis of thiocyanatoiron:

    Fe3+(aq) + SCN-(aq) ↔ [Fe(SCN)]2+(aq)

    [Fe(SCN)]2+ is a red-orange color. Fe3+ is pale yellow and SCN- is colorless.

  • Use Le Chatelier’s principle to predict how the color will change if more reactants are added. Why?

  • Use Le Chatelier’s principle to predict how the color will change if some reactants are taken away. Why?


Independent practice

Independent Practice

  • Assignment:

    • Choice 1: Complete all Reactions Rates & Equilibrium handouts and book HW. (Basic or Beginner Choice)

    • Choice 2: Equilibrium Article and questions (Proficient or Intermediate)

    • Choice 3: Challenge Assignment (Gibbs Free Energy or Calculating Reaction Rates – See “Challenge Zone” For page numbers).

Homework: Read pp. 512- 518, pp. 518 #1, 2, 3,6, 9; pp. 522 #18, 19, 20, 21, 23

  • Expectations:

    • You may 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.


Exit slip http tinyurl com boonchem15

Exit Slip: http://tinyurl.com/boonchem15

  • 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: Read pp. 512- 518, pp. 518 #1, 2, 3,6, 9; pp. 522 #18, 19, 20, 21, 23


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