Question

Explain Le-chatelier's principle. With suitable example.​

Answer 1

Answer:

Le Chatelier’s principle can be used to predict the behavior of a system due to changes in pressure, temperature, or concentration.

For example, if the pressure in a system increases, or the volume decreases, the equilibrium will shift to favor the side of the reaction that involves fewer moles of gas. Similarly, if the volume of a system increases, or the pressure decreases, the production of additional moles of gas will be favored.

Answer 2

Le-chatelier's principle

If a chemical reaction is at equilibrium and experiences a change in pressure, temperature, and concentration of product or reactant, the equilibrium shifts in the direction that tends to undo the change.

1. effect of concentration :

• If we increase the reactant, the reaction will proceed to produce more product, hence it will move in the forwarding direction.
• If we increase the product, the reaction will proceed to produce more reactants, hence it will move in the backward direction.

2. effect of pressure :

• As pressure is directly proportional to the number of moles
• As we increase pressure, the reaction will move where there are fewer moles.

3. effect of addition of inert gas:

• At constant pressure: equilibrium will shift towards more number of gas moles as it will increase the vessel`s volume
• At constant volume: it will not affect the equilibrium.

4. effect of temperature:

• On increasing, temperature equilibrium will shift towards an endothermic reaction
• Exothermic reactions are favored at low temperature
• Endothermic reactions are favored at high temperature

5. effect of catalyst :

• It doesn't affect the equilibrium
• It only increases the rate of reaction and decreases the activation energy of a reaction.

eg: $H_{2} + I_{2}$ ⇒ $2HI$ + heat

1. If we increase the concentration $HI$, the reaction will move in the backward direction.

2. If we increase the pressure, the reaction will have no effect as the number of moles on both sides is equal.

3. If we increase the temperature, the exothermic reaction will move in a backward direction producing more reactants.

4. If we add a catalyst, the equilibrium will not change.

Hence, the equilibrium will shift in the direction that tends to undo the change caused by factors.

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