What is meant by equilibrium shift towards larger numbers of moles?
This can be understood by using Le Chatelier Principle. The principle states that, if the equilibrium is disturbed by change in concentration, pressure or temperature, the equlibrium will shift in the direction, to balance the change.
Now pressure and number of moles are related to each other in terms of equilibrium. Higher the number of moles , more will be number of collision and hence more will be the pressure. In terms of chemical equilibrium :
An increase in pressure means increase the number of moles causes the system to shift in the direction of fewer number of moles. A decrease in pressure means lesser number of moles causes the system to shift in the direction of higher number of moles of particles.
If the number of moles of product is lesser than reactant, the equilibrium will favour in direction of products by increasing pressure.
For example :
N2 (g) + 3H2 (g) → 2NH3( g)
1 mol + 3 mol → 2 mol
If we increase the pressure , the reaction will favour the forward direction to decrease the overall pressure of the system means equilibrium will shift towards the lesser number of molecule.
If we decrease the pressure, the reaction will favour the backward direction to increase the overall pressure of the system by producing more number of molecules means equilibrium will shift towards the larger number of molecules.
Now pressure and number of moles are related to each other in terms of equilibrium. Higher the number of moles , more will be number of collision and hence more will be the pressure. In terms of chemical equilibrium :
An increase in pressure means increase the number of moles causes the system to shift in the direction of fewer number of moles. A decrease in pressure means lesser number of moles causes the system to shift in the direction of higher number of moles of particles.
If the number of moles of product is lesser than reactant, the equilibrium will favour in direction of products by increasing pressure.
For example :
N2 (g) + 3H2 (g) → 2NH3( g)
1 mol + 3 mol → 2 mol
If we increase the pressure , the reaction will favour the forward direction to decrease the overall pressure of the system means equilibrium will shift towards the lesser number of molecule.
If we decrease the pressure, the reaction will favour the backward direction to increase the overall pressure of the system by producing more number of molecules means equilibrium will shift towards the larger number of molecules.