In which of the following reactions, the concentration of product is higher than the concentration of reactant at equilibrium? (K = equilibrium constant)

Options

A. `A rarr B`, K = 0.001
B. `M rarr N`,K = 10
C. `X rarr Y`, K = 0.005
D. `R rarr P`, K = 0.01

Explanation

To determine in which of the given reactions the concentration of products is higher than the concentration of reactants at equilibrium, we need to analyze the equilibrium constant (K) for each reaction. The equilibrium constant is defined as follows:

\[ K = \frac{[\text{Products}]^{\text{stoichiometric coefficient}}}{[\text{Reactants}]^{\text{stoichiometric coefficient}}} \]

### Step-by-Step Solution:

1. **Understanding the Equilibrium Constant (K)**:
- The equilibrium constant (K) indicates the ratio of the concentrations of products to reactants at equilibrium.
- If \( K > 1 \), it implies that at equilibrium, the concentration of products is greater than that of reactants.
- If \( K < 1 \), it implies that at equilibrium, the concentration of reactants is greater than that of products.

2. **Analyzing the Options**:
- We will examine each of the provided reactions to determine the value of K.
- For each reaction, we will check if \( K > 1 \).

3. **Calculating K for Each Reaction**:
- Let's denote the reactions as follows:
- Reaction 1: \( aA \rightleftharpoons bB \) with \( K_1 \)
- Reaction 2: \( cC \rightleftharpoons dD \) with \( K_2 \)
- Reaction 3: \( eE \rightleftharpoons fF \) with \( K_3 \)
- Reaction 4: \( gG \rightleftharpoons hH \) with \( K_4 \)
- For each reaction, calculate K using the formula:
- \( K_1 = \frac{[B]^b}{[A]^a} \)
- \( K_2 = \frac{[D]^d}{[C]^c} \)
- \( K_3 = \frac{[F]^f}{[E]^e} \)
- \( K_4 = \frac{[H]^h}{[G]^g} \)

4. **Identifying the Correct Reaction**:
- After calculating K for each reaction, identify which reaction has \( K > 1 \).
- The reaction with \( K > 1 \) indicates that the concentration of products is higher than that of reactants at equilibrium.

5. **Conclusion**:
- Based on the calculations, select the reaction(s) where \( K > 1 \) as the answer to the question.