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In a gaseous reversible reaction
N2 (g) + O2 (g) ⇌ 2NO(g)+ heat
if pressure is increased, then the equilibrium constant would be :
- a)unchanged
- b)increased
- c)decreased
- d)sometimes increased, sometimes decreased
Correct answer is option 'A'. Can you explain this answer?
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In a gaseous reversible reactionN2 (g) + O2 (g) ⇌ 2NO(g)+ heatif pre...
N2 (g) + O2 (g) ⇌ 2NO(g)+ heat
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No. of moles of reactants = No. of moles of products.
The reaction in which number of moles of reactants are equal to number of moles of products are not affected by change in pressure (Le-Chatelier's principle).
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In a gaseous reversible reactionN2 (g) + O2 (g) ⇌ 2NO(g)+ heatif pre...
Pressure and Equilibrium Constant
Pressure is one of the factors that can affect the equilibrium of a reversible reaction. The equilibrium constant, denoted as K, is a measure of the extent to which a reaction proceeds. It is defined as the ratio of the concentrations of the products to the concentrations of the reactants at equilibrium, with each concentration raised to the power of its coefficient in the balanced chemical equation.
Effect of Pressure
When the pressure is increased, the equilibrium position of a reaction will shift in a way that reduces the total number of moles of gas. This is known as Le Chatelier's principle, which states that if a system at equilibrium is subjected to a change, the system will react in a way that opposes the change.
In the given reaction, the total number of moles of gas decreases from left to right. On the reactant side, we have one mole of N2 and one mole of O2, while on the product side, we have two moles of NO.
Impact on Equilibrium Constant
Since increasing the pressure reduces the total number of moles of gas, the equilibrium will shift towards the side with fewer moles of gas to counteract this change. In this reaction, the equilibrium will shift towards the left, favoring the formation of N2 and O2 from the products, NO.
The equilibrium constant, however, remains unchanged. This is because the equilibrium constant is a ratio of the concentrations of the products to the concentrations of the reactants, and the concentration of each species is influenced by the equilibrium position. As the equilibrium shifts towards the left, the concentrations of N2 and O2 increase, while the concentration of NO decreases. Despite these changes, the ratio of the concentrations remains constant, resulting in an unchanged equilibrium constant.
Conclusion
In summary, when the pressure is increased in a reversible reaction, the equilibrium position shifts towards the side with fewer moles of gas. However, this shift does not affect the equilibrium constant, which remains unchanged. Therefore, the correct answer is option 'A' - the equilibrium constant is unchanged.
Pressure is one of the factors that can affect the equilibrium of a reversible reaction. The equilibrium constant, denoted as K, is a measure of the extent to which a reaction proceeds. It is defined as the ratio of the concentrations of the products to the concentrations of the reactants at equilibrium, with each concentration raised to the power of its coefficient in the balanced chemical equation.
Effect of Pressure
When the pressure is increased, the equilibrium position of a reaction will shift in a way that reduces the total number of moles of gas. This is known as Le Chatelier's principle, which states that if a system at equilibrium is subjected to a change, the system will react in a way that opposes the change.
In the given reaction, the total number of moles of gas decreases from left to right. On the reactant side, we have one mole of N2 and one mole of O2, while on the product side, we have two moles of NO.
Impact on Equilibrium Constant
Since increasing the pressure reduces the total number of moles of gas, the equilibrium will shift towards the side with fewer moles of gas to counteract this change. In this reaction, the equilibrium will shift towards the left, favoring the formation of N2 and O2 from the products, NO.
The equilibrium constant, however, remains unchanged. This is because the equilibrium constant is a ratio of the concentrations of the products to the concentrations of the reactants, and the concentration of each species is influenced by the equilibrium position. As the equilibrium shifts towards the left, the concentrations of N2 and O2 increase, while the concentration of NO decreases. Despite these changes, the ratio of the concentrations remains constant, resulting in an unchanged equilibrium constant.
Conclusion
In summary, when the pressure is increased in a reversible reaction, the equilibrium position shifts towards the side with fewer moles of gas. However, this shift does not affect the equilibrium constant, which remains unchanged. Therefore, the correct answer is option 'A' - the equilibrium constant is unchanged.
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In a gaseous reversible reactionN2 (g) + O2 (g) ⇌ 2NO(g)+ heatif pressure is increased, then the equilibrium constant would be :a)unchangedb)increasedc)decreasedd)sometimes increased, sometimes decreasedCorrect answer is option 'A'. Can you explain this answer?
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