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Equilibrium Constant in Gaseous Systems Video Lecture - NEET
FAQs on Equilibrium Constant in Gaseous Systems Video Lecture - NEET
| 1. What is the equilibrium constant in gaseous systems? |  |
Ans. The equilibrium constant in gaseous systems, denoted as Kc, is a mathematical expression that relates the concentrations of reactants and products at equilibrium in a chemical reaction. It is determined by the ratio of the product concentrations raised to their stoichiometric coefficients divided by the reactant concentrations raised to their stoichiometric coefficients.
| 2. How is the equilibrium constant calculated in gaseous systems? | |
Ans. The equilibrium constant in gaseous systems can be calculated by analyzing the balanced chemical equation for the reaction and determining the concentrations of the reactants and products at equilibrium. The concentrations are then substituted into the equilibrium constant expression to obtain the numerical value of Kc.
| 3. What does the value of the equilibrium constant indicate in gaseous systems? | |
Ans. The value of the equilibrium constant in gaseous systems provides information about the extent of the reaction at equilibrium. If the value of Kc is greater than 1, it indicates that the reaction favors the formation of products. Conversely, if Kc is less than 1, it suggests that the reaction favors the presence of reactants. A value of Kc equal to 1 implies that the reactants and products are present in equal amounts at equilibrium.
| 4. How does the equilibrium constant change with temperature in gaseous systems? | |
Ans. The equilibrium constant in gaseous systems is temperature-dependent. As the temperature increases, the value of Kc may either increase or decrease, depending on the reaction. In an exothermic reaction, where heat is released, an increase in temperature leads to a decrease in Kc. On the other hand, in an endothermic reaction, where heat is absorbed, an increase in temperature results in an increase in Kc.
| 5. Can the equilibrium constant be altered by changing the partial pressures of the gaseous reactants and products? | |
Ans. Yes, the equilibrium constant in gaseous systems can be altered by changing the partial pressures of the gaseous reactants and products. This is known as Le Chatelier's principle. By increasing the pressure, the equilibrium will shift in the direction that reduces the total number of moles of gas. Conversely, decreasing the pressure will cause the equilibrium to shift towards the direction that increases the total number of moles of gas. However, it is important to note that changing the partial pressures will not change the numerical value of the equilibrium constant, but only the position of the equilibrium.
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