Cette leçon contient 19 diapositives, avec quiz interactifs et diapositives de texte.
Éléments de cette leçon
Slide 1 - Diapositive
How are you feeling today?
😒🙁😐🙂😃
Slide 2 - Sondage
What's the complete name of this person?
Slide 3 - Question ouverte
If a change is made to a system at dynamic equilibrium, the position of equilibrium moves to ____________ this change.
A
minimise
B
increase
C
favor
Slide 4 - Quiz
Learning Objectives
define Le Chatelier’s principle
use Le Chatelier’s principle to deduce qualitatively the effects of changes in temperature, concentration, pressure or presence of a catalyst on a system at equilibrium
Slide 5 - Diapositive
Slide 6 - Diapositive
Le Chatelier's Principle
" If a change is made to a system at dynamic equilibrium, the position of equilibrium moves to minimize this change. "
Slide 7 - Diapositive
Factors affecting Equilibrium
change in concentration
change in temperature
change in pressure
Slide 8 - Diapositive
Slide 9 - Diapositive
Group Activity 1: Concentration
Suppose you have an equilibrium established between four substances A, B, C and D.
Slide 10 - Diapositive
Equilibrium Equation:
A + 2B C + D
Σ
⇌
Slide 11 - Diapositive
Guide Questions
What would happen if you changed the conditions by increasing the concentration of A?
What would happen if you changed the conditions by decreasing the concentration of A?
Slide 12 - Diapositive
Group Activity 2: Temperature
For this, you need to know whether heat is given out or absorbed during the reaction.
Slide 13 - Diapositive
Assume that our forward reaction is exothermic (heat is evolved):
A + 2B C + D H = -250 kJ mol-1
Σ
⇌
Δ
Slide 14 - Diapositive
Guide Questions
What would happen if you changed the conditions by increasing the temperature?
Suppose the system is in equilibrium at 300°C, and you increase the temperature to 500°C. How can the reaction counteract the change you have made? How can it cool itself down again?
What would happen if you changed the conditions by decreasing the temperature?
Slide 15 - Diapositive
Group Activity 3: Pressure
This only applies to reactions involving gases.
Slide 16 - Diapositive
Equilibrium Equation:
A(g) + 2B(g) C(g) + D(g)
Σ
⇌
Slide 17 - Diapositive
Guide Questions
What would happen if you changed the conditions by increasing the pressure?
What would happen if you changed the conditions by decreasing the pressure?
What happens if there are the same number of molecules on both sides of the equilibrium reaction?