How is le chateliers principle used in the haber process

And here increase in concentration of oxygen increases the rate of forward reaction. Above reaction indicate that formation of ozone takes place with decrease in volume. The reaction is endothermic, so increasing the temperature will favour forward reaction.

Due to increase in temperature heat will be absorbed by the reaction. From this reaction it is clear that, the reaction is endothermic and accompanied by no change in volume. And here increase in concentration of nitrogen or oxygen increases the rate of forward reaction. Above reaction indicate that formation of nitric oxide takes place with no change in volume. Hence pressure has no effect on the equilibrium.

From this reaction it is clear that, the reaction is exothermic and accompanied by decrease in volume. Due to use of more number of moles, the increase in concentration of nitrogen oxide has a prominent effect. Above reaction indicate that formation of nitrogen dioxide takes place with decrease in volume. Hence increase in pressure favour forward reaction. The reaction is exothermic, so decreasing the temperature will favour forward reaction. Due to the decrease in temperature heat will be removed from the reaction.

From this reaction it is clear that, the reaction is endothermic and accompanied by increase in volume. And here increase in concentration of phosphorous pentachloride increases the rate of forward reaction. Above reaction indicate that formation of nitrogen dioxide takes place with increase in volume. Hence decrease in pressure favour forward reaction. According to this principle, if a system at equilibrium is subjected to a disturbance or stress, then the equilibrium shifts in the direction that tends to nullify the effect of the disturbance or stress.

Let us consider the effects of changes in temperature, concentration and pressure, on the equilibrium reactions and the predictions of Le Chatelier's principle. Effect of change of concentration. Consider the following equilibrium reaction. At the equilibrium conditions the reaction mixture contains both the reactant and product molecules, that is, N 2 , O 2 and NO molecules.

The concentrations of reactant and product molecules are constant and remain the same as long as the equilibrium conditions are maintained the same. If a change is imposed on the system by purposely adding NO into the reaction mixture then the product concentration is raised. Since the system possesses equilibrium concentrations of reactants and products, the excess amount of NO react in the reverse direction to produce back the reactants and this results in the increase in concentrations of N 2 and O 2.

Similarly if the concentration of reactants such as N 2 and O 2 are purposely raised when the system is already in the state of equilibrium, the excess concentrations of N 2 and O 2 favour forward reaction. Concentration of NO is raised in the reaction mixture. In general, in a chemical equilibrium increasing the concentrations of the. Effect of change of temperature. A chemical equilibrium actually involves two opposing reactions.

One favouring the formation of products and the other favouring the formation of reactants. If the forward reaction in a chemical equilibrium is endothermic accompanied by absorption of heat then the reverse reaction is exothermic accompanied by evolution of heat. Let us consider the example. In this equilibrium, the reaction of the product formation NO 2 is endothermic in nature and therefore, the reverse reaction of reactant formation N 2 O 4 should be exothermic.

If the above equilibrium reaction mixture is heated then its temperature will be raised. According to Le Chatelier's principle, the equilibrium will shift in the direction which tends to undo the effect of heat. Therefore,the equilibrium will shift towards the formation of NO 2 and subsequently dissociation of N 2 O 4 increases.

Therefore, generally, when the temperature is raised in a chemical equilibrium, among the forward and reverse reactions, the more endothermic reaction will be favoured. Similarly, if the temperature of the. Effect of change of pressure. If a system in equilibrium consists of reactants and products in gaseous state, then the concentrations of all components can be altered by changing the total pressure of the system. Consider the equilibrium in the gaseous state such as.

Increase in the total pressure of the system in equilibrium will decrease the volume proportionately. If the forward reaction is exothermic, reducing the temperature favours the formation of the product.

The yield of the product will be increased. Increasing the system pressure by reducing the volume causes the equilibrium to shift to the side of the equation with the least number of gaseous molecules. Decreasing the system pressure by increasing the volume causes the equilibrium to shift to the side of the equation with the most number of gaseous molecules. Where there are equal numbers of molecules on the reactant and product sides, pressure has no effect on the position of the equilibrium.

Increasing the reactant concentration shifts the equilibrium to the right to make more products and to reduce the concentration of the added reactant. Decreasing the concentration of a reactant shifts the equilibrium to the left to make more of that reactant. Consequently the concentration of products decreases. Catalysts are useful because they lower the activation energy, and equilibrium is achieved faster.

This is important in industry as there are considerable savings to be made in time and energy as reactions can be conducted where appropriate at lower temperatures. However, nitrogen and hydrogen do not exist as single atom, they both exist as diatomic molecules held together by strong covalent bonds. Nitrogen molecules are held together by very strong triple covalent bonds and the single covalent bond between hydrogen atoms is also quite strong.