For a reversible reaction, if the concentrations of the reactants are doubled, then the equilibrium constant value

Options

A. Gets doubled
B. Gets halved
C. Remains the same
D. increases four times

Answer

To solve the question regarding the effect of doubling the concentrations of the reactants on the equilibrium constant, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Concept of Equilibrium Constant (K)**:
The equilibrium constant (K) for a reversible reaction 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.

\[ K = \frac{[Products]}{[Reactants]} \]

2. **Identify the Dependence of K**:
The equilibrium constant is dependent on temperature. This means that unless the temperature changes, the value of K remains constant regardless of changes in the concentrations of reactants or products.

3. **Analyze the Effect of Doubling Reactant Concentrations**:
If the concentrations of the reactants are doubled, we can express this mathematically. Let’s assume the initial concentrations of the reactants are [A] and [B]. If we double these concentrations, they become [2A] and [2B].

4. **Recalculate the Equilibrium Constant**:
When we double the concentrations of the reactants, the equilibrium constant does not change. It still remains dependent only on the temperature. Therefore, even after doubling the concentrations, the equilibrium constant K remains the same.

5. **Conclusion**:
Thus, the value of the equilibrium constant does not change when the concentrations of the reactants are doubled, provided the temperature remains constant.

### Final Answer:
The equilibrium constant value remains the same when the concentrations of the reactants are doubled.

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