Test: Factors Affecting Equilibrium (12 July) - JEE MCQ

Chemical equilibrium is the state of a system in which the concentration of reactants and products does not change over time, and the system is in a state of balance where the rate of the forward reaction is equal to the rate of the reverse reaction. This is a fundamental concept in chemistry.
Additional Fact: Chemical equilibrium is a dynamic process where molecules are constantly reacting, but at the macroscopic level, there is no net change in concentrations. It is represented using the equilibrium constant, K.

According to Le-Chatelier's principle, when the temperature is increased for an exothermic reaction (heat is supplied), the equilibrium will shift in the direction that consumes heat, which is towards the reactants. This shift favors the exothermic reaction.
Additional Fact: Exothermic reactions release heat energy, while endothermic reactions absorb heat energy.

Increasing the concentration of one or more of the reactant species in a chemical equilibrium will shift the equilibrium towards the products. This is in accordance with Le-Chatelier's principle.
Additional Fact: Le-Chatelier's principle helps predict how changes in conditions affect chemical equilibria, including changes in concentration.

The effect of increasing pressure on a gaseous reaction in equilibrium depends on the number of moles of gas on each side of the reaction. If the number of moles of gas on the reactant's side is greater, increasing pressure will shift the equilibrium towards the products, and vice versa.
Additional Fact: Le-Chatelier's principle helps determine the direction of the shift in equilibrium.

A catalyst is used in a chemical reaction to speed up both forward and reverse reactions without affecting the equilibrium position. It lowers the activation energy required for the reaction to occur, allowing the reaction to reach equilibrium more quickly.
Additional Fact: Catalysts are essential in many industrial processes to increase reaction rates and efficiency.

When the volume of a gaseous mixture at equilibrium is reduced, the equilibrium shifts towards the side with fewer gaseous molecules. This often means a shift towards the products.
Additional Fact: Changes in volume can affect the equilibrium position in gaseous reactions.

Adding an inert gas at constant volume to an equilibrium system has no effect on the equilibrium. The concentrations of reactants and products remain unchanged.
Additional Fact: Inert gases are often used to maintain constant pressure during reactions without affecting the equilibrium position.

Adding an inert gas at constant pressure to an equilibrium system increases the volume of the system, which, in turn, decreases the number of moles of reactants and products per unit volume. As a result, the equilibrium shifts towards the side with more gaseous molecules.
Additional Fact: Changes in pressure can impact the equilibrium position in gaseous reactions.

The primary function of a catalyst in a chemical reaction is to speed up both forward and reverse reactions without changing the equilibrium position. It lowers the activation energy required for the reaction.
Additional Fact: Catalysts are crucial in various industries to improve reaction efficiency.

When a system is in a state of dynamic equilibrium, it means that the rate of the forward reaction equals the rate of the reverse reaction, and there is no net change in the concentrations of reactants and products over time.
Additional Fact: Dynamic equilibrium is a key concept in chemistry, often associated with chemical reactions.