The equilibrium constant for a reaction is K, and the reaction quotient is Q . For a particular reaction mixture , the ration `(K)/(Q)` is 0.33. this means that:

Options

A. the reaction mixture will equilirate to from more reactant species
B. the rection mixture will equilirate to from more product species
C. the equlibrium ratio of reactant to product concentration will be 3
D. the equilibrium ratio of reactant to product concentrations will be 0.33

Answer

To solve the problem, we need to analyze the relationship between the equilibrium constant (K) and the reaction quotient (Q).

### Step-by-Step Solution:

1. **Understanding K and Q**:
- The equilibrium constant (K) is a value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature.
- The reaction quotient (Q) is calculated using the same formula as K, but it can be determined at any point in time during the reaction, not just at equilibrium.

2. **Given Information**:
- We are given that the ratio \( \frac{K}{Q} = 0.33 \).

3. **Analyzing the Ratio**:
- Since \( \frac{K}{Q} = 0.33 \), we can infer that \( K < Q \) because the ratio is less than 1.

4. **Implication of K < Q**:
- When \( Q > K \), it indicates that the concentration of products is greater than what it would be at equilibrium.
- Therefore, the reaction will shift to the left (backward direction) to form more reactants in order to reach equilibrium.

5. **Conclusion**:
- Since the reaction will proceed in the backward direction, it means that the reaction mixture will equilibrate to form more reactant species.

### Final Answer:
The correct conclusion is that the reaction mixture will equilibrate to form more reactant species.

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