Le Chatelier's Principle

This lesson covers:

  1. What 'Le Chatalier's principle' is
  2. How temperature affects the position of equilibrium
  3. How pressure affects the position of equilibrium
  4. How concentration affects the position of equilibrium

Le Chatelier's principle states that if you change the conditions of a r reaction, the position of e will shift to try and c the change.

eversible
quilibrium
ounteract

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At equilibrium, if there are more products than reactants, we say that the position of equilibrium lies:

In the middle

To the right

To the left

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What are the three factors that affect the position of equilibrium?


(Press continue when you're ready to check your answer)

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Diagram showing the shift in equilibrium position with an increase in pressure.

An increase in pressure moves the position of equilibrium to whichever side has the:

smaller number of gas molecules

larger number of gas molecules

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In a reversible reaction, changes in pressure will only affect substances that are in the:

liquid state

gaseous state

solid state

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increases / decreases


Le Chatalier's principle states that if you increase the pressure, the position of equilibrium will shift to the side that the pressure back down. 

decreases

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N2(g) + 3H2(g) ⇋ 2NH3(g)


In the above reaction, increasing the pressure will:

Shift the position of equilibrium to the left

Have no effect on the position of equilibrium

Shift the position of equilibrium to the right

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H2(g) + I2(g) ⇋ 2HI(g)


In the above reaction, increasing the pressure will:

Shift the position of equilibrium to the left

Shift the position of equilibrium to the right

Have no effect on the position of equilibrium

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2NO2(g) ⇋ N2O4(g) (-24 kJ mol-1)


In the reaction above, the (-24 kJ mol-1) tells us that the forward reaction is:

Exothermic

Endothermic

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2NO2(g) ⇋ N2O4(g) (-24 kJ mol-1)


In the above reaction, increasing the temperature will:

Shift the position of equilibrium to the right

Have no effect on the position of equilibrium

Shift the position of equilibrium to the left

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N2(g) + 3H2(g) ⇋ 2NH3(g)


For the above reaction, increasing the concentration of nitrogen will:

Have no effect on the position of equilibrium

Shift the position of equilibrium to the left

Shift the position of equilibrium to the right

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