| Method |
Precise Learning Objective |
Linked |
Question / Activity
(Designed for maximum working out) |
Stepping Stones |
Pitstop Check
(Thinking Map) |
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If the temperature of a system at equilibrium is increased:
- the relative amount of products at equilibrium increases for an endothermic reaction
- the relative amount of products at equilibrium decreases for an exothermic reaction. |
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What would happen if the temperature was increased for the reaction below:
N2(g) 3H2(g) (reversible reaction) 2NH3(g)
The forward reaction is exothermic. Demo 1:
The equilibrium of the cobalt chloride–water system;
temperature. Observe colour of reaction at different temperatures (20,30,40 degrees) |
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If the temperature of a system at equilibrium is decreased:
- the relative amount of products at equilibrium decreases for an endothermic reaction
- the relative amount of products at equilibrium increases for an exothermic reaction. |
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What would happen if the temperature was decreased for the reaction below:
N2(g) 3H2(g) (reversible reaction) 2NH3(g)
The forward reaction is exothermic. demo of co |
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Students should be able to interpret appropriate given data to predict the effect of a change in temperature on given reactions at equilibrium. |
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Does increasing the temperature of a reaction favor the endothermic or exothermic reaction? |
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When a reversible reaction occurs in apparatus which prevents the escape of reactants and products, equilibrium is reached when the forward and reverse reactions occur at exactly the same rate. |
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What does the term equilibrium mean? Watch https://www.youtube.com/watch?v=dUMmoPdwBy4 |
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Students should be able to interpret appropriate given data to predict the effect of pressure changes on given reactions at equilibrium. |
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When does changing the pressure of gaseous reactions not affect the equilibrium? Go Further: complete the Haber process worksheet. |
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For gaseous reactions at equilibrium:
? an increase in pressure causes the equilibrium position to shift towards the side with the smaller number of molecules as shown by the symbol equation for that reaction
? a decrease in pressure causes the equilibrium position to shift towards the side with the larger number of molecules as shown by the symbol equation for that reaction. |
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How does increasing and decreasing the pressure for gaseous reactions at equilibrium? |
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The relative amounts of all the reactants and products at equilibrium depend on the conditions of the reaction. |
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What does the relative amounts of all the reactants and products at equilibrium depend on? Ask students what happens when a bottle of coke is opened -> bubbles fizz out -> why? Affect of pressure on carbonic acid reversible reactions. |
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If a system is at equilibrium and a change is made to any of the conditions, then the system responds to counteract the change. |
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What happens when a system is at equilibrium and a change is made to the conditions? Watch the two videos and annotate the snap shots (hand outs - video 1 and video 2 in shared folder):
https://www.youtube.com/watch?v=7zuUV455zFs
https://www.youtube.com/watch?v=XhQ02egUs5Y
Go further: Write the correct sentences for the sentence exerts (shared area). |
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The effects of changing conditions on a system at equilibrium can be predicted using Le Chatelier's Principle. |
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What is Le Chatelier's principle used for? |
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Students should be able to make qualitative predictions about the effect of changes on systems at equilibrium when given appropriate information. |
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How would changing the conditions of the equation below effect the equilibrium?
A(g) 2B (g) (reversible arrow) C(g) D(g)
a) increasing concentration of A
b) increasing the pressure of the reactants
c) increasing the temperature of the reaction (the forward reaction is exothermic) Complete dynamic equilibrium worksheet. |
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If the concentration of one of the reactants or products is changed, the system is no longer at equilibrium and the concentrations of all the substances will change until equilibrium is reached again. |
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What happens when the concentration of one of the reactions or products in an equilibrium system is changed? |
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If the concentration of a reactant is increased, more products will be formed until equilibrium is reached again. |
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What happens when the concentration of a reactant is increased in an equilibrium system? |
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If the concentration of a product is decreased, more reactants will react until equilibrium is reached again. |
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What happens when the concentration of a reactant is decreased in an equilibrium system? |
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Students should be able to interpret appropriate given data to predict the effect of a change in concentration of a reactant or product on given reactions at equilibrium. |
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What would happen if the concentration of potassium chloride is increase?
Cl2(g) H2O(l) (reversible arrow) Cl-(aq) ClO-(aq) 2H (aq) |
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