Question

Given the following reaction:

2N₂O₃ (g) ç==è 2NO₂ (g) + O₂ (g) Delta H = 322 KJ

State which way the equilibrium will shift under the following conditions:

Lower temp

Higher volume

Condense N₂O₃

Add O₂

Answer 1

1)

Forward reaction is endothermic in nature

we are decreasing temperature or removing heat here

so, according to Le Chatelier's principle,

equilibrium will move in direction which release heat

hence, backward reaction will be favoured

Answer: Equilibrium moves to reactant side

2)

We are increasing volume here

In other words we are trying to decrease pressure

so, according to Le Chatelier's principle,

Reaction will try to increase the pressure

Hence it will move in a direction which have more gaseous molecules

Here reactant has more gaseous molecule

So equilibrium will move to left

Answer: Equilibrium moves to reactant side

3)

This is like removing a reactant

According to Le Chatelier's Principle,

Removing reactant will shift reaction towards reactant side

Answer: Equilibrium moves to reactant side

4)

we are adding a product

According to Le Chatelier's Principle,

Adding product will shift reaction towards reactant side

Answer: Equilibrium moves to reactant side