7.7 CW - Equilibrium and Le Chatelier's Principle

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In order for a system to reach equilibrium, it must be a ​

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change occurring in a ​

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system. It will meet ​

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equilibrium when the rates of the forward and reverse reactions are ​

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​ and the concentration of the reactants and products are

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.

Multiple Choice

When a reversible reaction is at equilibrium, the concentration of the products and the concentration of the reactants must be

• increasing

• decreasing

• constant

• equal

Multiple Choice

What occurs when a reaction reaches equilibrium?

• The concentration of the reactants increases.

• The concentration of the products increases.

• The rate of the forward reaction is equal to the rate of the reverse reaction.

• The rate of the forward reaction is slower than the rate of the reverse reaction.

Multiple Choice

Given the diagram representing a closed system at constant temperature:

Which statement describes this system at equilibrium?

• The mass of H₂O (l) equals the mass of H₂O (g).

• The volume of H₂O (l) equals the volume of H₂O (g).

• The number of moles of H₂O (l) equals the number of moles of H₂O (g).

• The rate of evaporation of H₂O (l) equals the rate of condensation of H₂O (g).

• Rewatch the video to recap how changing the concentration of a Reactant or Product effects chemical equilibrium.

• Watch the end to see how changes in pressure effect chemical equilibrium.

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N₂ + 3H₂ ⇄ 2NH₃



If the concentration of N₂ is INCREASED the reaction shifts toward the ​

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N₂ + 3H₂ ⇄ 2NH₃



If the concentration of NH₃ is DECREASED the reaction shifts toward the ​ ​

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​

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N₂ + 3H₂ ⇄ 2NH₃



If the concentration of NH₃ is INCREASED the reaction shifts toward the ​ ​

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and the concentration of N₂ ​

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.

Multiple Choice

2SO₂(g)  +  O₂(g)  ⇄  2SO₃(g)  +  energy

Which change causes the equilibrium to shift to the right?

• adding more SO₃

• removing O₂

• adding more O₂

• removing SO₂

Multiple Choice

2SO₂(g)  +  O₂(g)  ⇄  2SO₃(g)  +  energy

What happens to the concentration of SO₃ when more O₂ is added to the reaction at equilibrium.

• The concentration of SO₃ increases.

• The concentration of SO₃ decreases.

• The concentration of SO₃ remains constant.

Multiple Choice

2SO₂(g)  +  O₂(g)  ⇄  2SO₃(g)  +  energy

What happens to the concentration of SO₃ when SO₂ is removed from the system after it reaches equilibrium at equilibrium.

• The concentration of SO₃ increases.

• The concentration of SO₃ decreases.

• The concentration of SO₃ remains constant.

• Watch the rest of this video to see how changes in pressure will effect a system at equilibrium.

• Pay close attention to the AMOUNT of gas particles.

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An INCREASE in pressure will push/shift the system towards the side of the reaction with ​

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gas particles because there is a ​

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in volume.

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A DECREASE in pressure will push/shift the system towards the side of the reaction with ​ ​

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gas particles because there is an ​

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in volume.

Multiple Choice

2SO₃(g)  ⇌   2SO₂(g) + O₂(g)

Increasing the pressure on the system will shift the equilibrium towards the

• reactants and the concentration of O₂ increases.

• products and the concentration of O₂ increases.

• reactants and the concentration of O₂ decreaes.

• products and the concentration of O₂ decreases.

Poll

How do you feel about Le Chatelier's Principle-based questions?

• Super good - I think they are pretty easy.

• Sorta good - I think I got it.

• Meh - I'm still confused.

• Okay - I think I just need more practice.