Question

chemical equilibrium between gaseous reactants and products is shown.

N2(g) + 3H2(g) ⇌ 2NH3(g)

How will the reaction be affected if the pressure on the system is decreased?

Answer 1

Answer:

The reaction is shifted to the left.

Explanation:

• Le Châtelier's principle states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.

• When there is a decrease in pressure, the equilibrium will shift towards the side with more no. of moles of gas molecules of the reaction.

• The reactants side (left) has 4.0 moles of gases and the products side (right) has 2.0 moles of gases.

• So, decreasing the pressure will shift the reaction to the side with more moles of gas (left side).

• so, the reaction is shifted to the left.

Answer 2

When the pressure is decreased, the equilibrium will shift to the left hand side where there are more volumes.

We know that when a constraint is imposed on a reaction system in equilibrium, the equilibrium position is adjusted so as to annul the constraint.

This constraint could be a change in temperature, pressure, volume or concentration. When the pressure is decreased, the equilibrium will shift to the left hand side where there are more volumes.

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