Question

The chemical system shown below is at equilibrium. Which change in conditions will not result in a spontaneous forward reaction? N2(g) + 3 H2(g) ⇌ 2 NH3(g) Kp = 4 × 105

adding more N2

reducing the pressure

reducing the volume

decreasing the NH3

Answer 1

According to Le Chatelier principle, if we add or reduced some substance,then system will re-established the equilibrium in such a so that it can minimise the effect.

If we add N2 ,so to minimise it's effect product formation will be more ,i.e, spontaneous in forward reaction

If we reduce pressure then equilibrium shift to that Direction in which it has more moles of gases,i.e, spontaneous in backward reaction

If we reduce Volume,then equilibrium shift in that direction in which it has lesser number of moles,i.e, spontaneous to forward reaction.

Decreasing NH3, shift the equilibrium to right direction,i.e spontaneous to forward reaction.

ans: reducing pressure, will not results in a spontaneous forward reaction