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Equilibrium in Chemical Processes Video Lecture | Chemistry Class 11 - NEET

FAQs on Equilibrium in Chemical Processes Video Lecture - Chemistry Class 11 - NEET

1. What is chemical equilibrium in a chemical process?

Ans.Chemical equilibrium refers to the state in a reversible reaction where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. This dynamic balance means that although the reactions are still occurring, there is no net change in the amounts of substances involved.

2. How can Le Chatelier's principle be applied to predict changes in equilibrium?

Ans.Le Chatelier's principle states that if an external change is applied to a system at equilibrium, the system adjusts to counteract that change and restore a new equilibrium. For example, if the concentration of a reactant is increased, the equilibrium will shift to favor the formation of products, thus reducing the concentration of the added reactant.

3. What factors affect the position of equilibrium in a chemical reaction?

Ans.The position of equilibrium can be affected by several factors including changes in concentration of reactants or products, temperature, and pressure (for gaseous reactions). Increasing the concentration of reactants typically shifts the equilibrium to the right (towards products), while increasing temperature may favor the endothermic reaction.

4. How does temperature influence chemical equilibrium?

Ans.Temperature changes can shift the position of equilibrium depending on whether the reaction is exothermic or endothermic. For endothermic reactions, increasing the temperature will favor the formation of products, while for exothermic reactions, increasing the temperature will favor the reactants.

5. What is the significance of the equilibrium constant (K) in chemical reactions?

Ans.The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. A large K value indicates that products are favored at equilibrium, while a small K value indicates that reactants are favored. This helps predict how changes in conditions will affect the equilibrium position.

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Oct 15, 2025 Last updated

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