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In a reversible chemical reaction at equilibrium, if the concentration of any one of the reactants is doubled, then the equilibrium constant will
- a)also be doubled
- b)be halved
- c)remain the same
- d)become one-fourth
Correct answer is option 'C'. Can you explain this answer?
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In a reversible chemical reaction at equilibrium, if the concentration...
Equilibrium constant do not depend upon concentration of product or reactant so , it will remain the same.
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In a reversible chemical reaction at equilibrium, if the concentration...
Understanding Equilibrium Constant
In a reversible chemical reaction, the equilibrium constant (K) is defined as the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their respective coefficients in the balanced equation.
Equilibrium Expression
For a general reaction:
\[ aA + bB \rightleftharpoons cC + dD \]
The equilibrium constant \( K \) is given by:
\[ K = \frac{[C]^c[D]^d}{[A]^a[B]^b} \]
Where:
- [A], [B], [C], [D] are the equilibrium concentrations of the respective substances.
- a, b, c, d are the stoichiometric coefficients.
Effect of Doubling a Reactant's Concentration
When the concentration of one of the reactants (e.g., [A]) is doubled, it changes the concentrations at that moment but does not alter the equilibrium constant \( K \). Instead:
- The system will shift to re-establish equilibrium.
- The concentrations of products will adjust to maintain the ratio defined by \( K \).
Key Points
- Equilibrium Constant Independence: \( K \) is a constant at a given temperature, regardless of the concentrations of reactants or products.
- Reaction Shift: While concentrations change, the overall ratio defining \( K \) remains unchanged as the system adjusts.
Conclusion
Therefore, even if the concentration of a reactant is doubled, the equilibrium constant \( K \) will remain the same (option C). This is a fundamental principle of chemical equilibria, emphasizing the constancy of \( K \) at a specific temperature.
In a reversible chemical reaction, the equilibrium constant (K) is defined as the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their respective coefficients in the balanced equation.
Equilibrium Expression
For a general reaction:
\[ aA + bB \rightleftharpoons cC + dD \]
The equilibrium constant \( K \) is given by:
\[ K = \frac{[C]^c[D]^d}{[A]^a[B]^b} \]
Where:
- [A], [B], [C], [D] are the equilibrium concentrations of the respective substances.
- a, b, c, d are the stoichiometric coefficients.
Effect of Doubling a Reactant's Concentration
When the concentration of one of the reactants (e.g., [A]) is doubled, it changes the concentrations at that moment but does not alter the equilibrium constant \( K \). Instead:
- The system will shift to re-establish equilibrium.
- The concentrations of products will adjust to maintain the ratio defined by \( K \).
Key Points
- Equilibrium Constant Independence: \( K \) is a constant at a given temperature, regardless of the concentrations of reactants or products.
- Reaction Shift: While concentrations change, the overall ratio defining \( K \) remains unchanged as the system adjusts.
Conclusion
Therefore, even if the concentration of a reactant is doubled, the equilibrium constant \( K \) will remain the same (option C). This is a fundamental principle of chemical equilibria, emphasizing the constancy of \( K \) at a specific temperature.
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In a reversible chemical reaction at equilibrium, if the concentration of any one of the reactants is doubled, then the equilibrium constant willa)also be doubledb)be halvedc)remain the samed)become one-fourthCorrect answer is option 'C'. Can you explain this answer?
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