Question

how would be effect of equilibrium on temperature pressure and concentration

Answer 1

Le Chatlier’s principle states that if a reaction at equilibrium is perturbed by a change in conditions like concentration of the substances taking part in the reaction, volume, pressure or temperature, then the system adjusts to the change so as to minimize the impact of the change and re-establishes equilibrium state.
For example, the reaction N2 + 3H2 ⇔ 2NH3 ΔH = -ve (exothermic reaction)

Concentrations of substances taking part in the reaction. If the concentration of N2 and H2 are increased. This disturbs the equilibrium state. To re-establish equilibrium state, the added N2 and H2 need to be utilized and that is possible if the reaction proceeds in the forward direction to consume the added nitrogen and hydrogen gas. Addition of ammonia moves the reaction in the left or reverse direction.

Temperature: Increasing temperature implies heat is added. An endothermic reaction requires heat and can use up extra energy supplied to the system. The reverse reaction, decomposition of ammonia to nitrogen and hydrogen gas is endothermic and will be favoured at high temperature. The synthesis of ammonia is favoured at low temperatures.

Pressure and volume: Pressure and volume of a gas are inversely related. So, if volume is high, pressure is low. In the above reaction, there are 4 moles of gases on the right side which form 2 moles of ammonia. So, volume is less on right side or ammonia side and this side has a higher pressure. Therefore, increase in pressure favours the forward direction.