Which reaction is favoured when temperature increases?

The side with less moles of gas

What happens when pressure changes and both sides have equal moles of gas?

The position of equilibrium does not shift

What happens when the concentration of a product increases?

Equilibrium shifts left, using up some of the added product.

What happens when a product is removed e.g H ions reacting with NaOH that has been added,

Equilibrium shifts right, replacing some of the removed H ion product.

What does K > 1 tell you?

The reaction favours the products.

Does a large value of K mean the reaction is very fast?

No. K indicates the equilibrium position, not the reaction rate.

For an exothermic forward reaction, what happens to the equilibrium position and K when temperature decreases?

Equilibrium shifts right and K increases.

For an endothermic forward reaction, what happens to the equilibrium position and K when temperature increases?

Equilibrium shifts right and K increases.

What happens to the equilibrium position and K when a product is added at constant temperature?

Equilibrium shifts left, consuming some of the added product. K remains unchanged.

What happens to the equilibrium position and K when a reactant is added at constant temperature?

Equilibrium shifts right, consuming some of the added reactant. K remains unchanged.

What happens to the equilibrium position and K when pressure decreases?

Equilibrium shifts towards more moles of gas. K remains unchanged.

2SO₂(g) + O₂(g) ⇌ 2SO₃(g), ΔH < 0. What happens to SO₃ yield and K when temperature increases?

SO₃ equilibrium yield decreases and K decreases. Equilibrium shifts left.

N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Write K

K = [NH₃]² / ([N₂][H₂]³).

Predict the effect of increasing pressure on K and equilibrium position N₂(g) + 3H₂(g) ⇌ 2NH₃(g

Equilibrium shifts right because gas moles decrease from 4 to 2. K is unchanged.

What happens to the equilibrium position and K when a product is removed at constant temperature?

Equilibrium shifts right, replacing some of the removed product. K remains unchanged.

What does K < 1 tell you?

The equilibrium favours reactants.

For an endothermic forward reaction, what happens to the equilibrium position and K when temperature increases?

Equilibrium shifts right and K increases.

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Equilibrium AH

Question	Answer
Are exothermic or endothermic forward reactions favoured when temperature increases?	endothermic
Which reaction is favoured when temperature increases?	The side with less moles of gas
What happens when pressure changes and both sides have equal moles of gas?	The position of equilibrium does not shift
What happens when the concentration of a product increases?	Equilibrium shifts left, using up some of the added product.
What happens when a product is removed e.g H ions reacting with NaOH that has been added,	Equilibrium shifts right, replacing some of the removed H ion product.
Does a catalyst change the equilibrium position?	No
For equilibrium to occur what must the system be.	Closed
What does K > 1 tell you?	The reaction favours the products.
Does a large value of K mean the reaction is very fast?	No. K indicates the equilibrium position, not the reaction rate.
For an exothermic forward reaction, what happens to the equilibrium position and K when temperature decreases?	Equilibrium shifts right and K increases.
For an endothermic forward reaction, what happens to the equilibrium position and K when temperature increases?	Equilibrium shifts right and K increases.
What happens to the equilibrium position and K when a product is added at constant temperature?	Equilibrium shifts left, consuming some of the added product. K remains unchanged.
What happens to the equilibrium position and K when a reactant is added at constant temperature?	Equilibrium shifts right, consuming some of the added reactant. K remains unchanged.
What happens to the equilibrium position and K when pressure decreases?	Equilibrium shifts towards more moles of gas. K remains unchanged.
Write the formula for K . H₂(g) + I₂(g) ⇌ 2HI(g)	[HI]2 / [H2] [I2]
How does a catalyst affect K	It does not affect K
2SO₂(g) + O₂(g) ⇌ 2SO₃(g), ΔH < 0. What happens to SO₃ yield and K when temperature increases?	SO₃ equilibrium yield decreases and K decreases. Equilibrium shifts left.
N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Write K	K = [NH₃]² / ([N₂][H₂]³).
Predict the effect of increasing pressure on K and equilibrium position N₂(g) + 3H₂(g) ⇌ 2NH₃(g	Equilibrium shifts right because gas moles decrease from 4 to 2. K is unchanged.
What happens to the equilibrium position and K when a product is removed at constant temperature?	Equilibrium shifts right, replacing some of the removed product. K remains unchanged.
What does K < 1 tell you?	The equilibrium favours reactants.
For an endothermic forward reaction, what happens to the equilibrium position and K when temperature increases?	Equilibrium shifts right and K increases.

Created by: brightminds

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