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1. What is equilibrium in the context of chemistry?
Ans. Equilibrium in chemistry refers to a state where the forward and reverse reactions occur at the same rate, resulting in a constant concentration of reactants and products. It is a dynamic state where there is no net change in the amounts of reactants and products.
2. How is equilibrium achieved in a chemical reaction?
Ans. Equilibrium is achieved in a chemical reaction when the rates of the forward and reverse reactions become equal. This can happen by adjusting the temperature, pressure, or concentration of reactants and products. Once equilibrium is reached, the concentrations of substances involved remain constant.
3. What are the factors that can shift the equilibrium of a chemical reaction?
Ans. Several factors can shift the equilibrium of a chemical reaction. These include changes in temperature, pressure, and concentrations of reactants and products. Additionally, the addition or removal of a catalyst or a change in the volume of the reaction vessel can also affect the equilibrium.
4. How does Le Chatelier's principle relate to equilibrium?
Ans. Le Chatelier's principle states that if an external stress is applied to a system at equilibrium, the system will adjust itself in such a way as to counteract the stress and restore equilibrium. This principle helps predict the direction in which the equilibrium will shift when changes are made to the conditions of a chemical reaction.
5. How can the equilibrium constant be used to determine the extent of a chemical reaction?
Ans. The equilibrium constant (K) is a numerical value that represents the ratio of product concentrations to reactant concentrations at equilibrium. It can be used to determine the extent of a chemical reaction by comparing the values of K for different reactions. A larger value of K indicates a higher concentration of products at equilibrium, suggesting a more complete reaction.
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