In the following reaction:
`2NO_((g))+Cl_(2(g))hArr2NOCl_((g))`
it is observed that equilibrium is not attained and the rate of forward reaction is greater than rate of backward reaction. Which of the following is true for the reaction ? (A) K p = Q p (B) Q p > K p (C) Q p < K p (D) Q p = 0

Options

A. `K_(p)=Q_(p)`
B. `Q_(p)gtK_(p)`
C. `Q_(p)ltK_(p)`
D. `Q_(p)=0`

Explanation

To solve the problem, we need to analyze the given reaction and the information provided about the rates of the forward and backward reactions.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
The reaction given is:
\[ 2NO_{(g)} + Cl_{2(g)} \rightleftharpoons 2NOCl_{(g)} \]
This is a reversible reaction where nitrogen monoxide (NO) and chlorine (Cl2) react to form nitrosyl chloride (NOCl).

2. **Equilibrium Concept**:
In a reversible reaction, equilibrium is attained when the rate of the forward reaction equals the rate of the backward reaction. At this point, the concentrations of reactants and products remain constant.

3. **Given Information**:
- It is stated that equilibrium is not attained.
- The rate of the forward reaction is greater than the rate of the backward reaction.

4. **Implications of the Given Information**:
Since the forward reaction is faster, this means that the concentration of products (NOCl) is increasing while the concentration of reactants (NO and Cl2) is decreasing. Therefore, we can conclude that the reaction is still moving towards the formation of more products.

5. **Understanding Reaction Quotient (Qp)**:
The reaction quotient \( Q_p \) is defined as:
\[ Q_p = \frac{(P_{NOCl})^2}{(P_{NO})^2 \cdot (P_{Cl2})} \]
where \( P \) represents the partial pressures of the respective gases.

6. **Comparing Qp and Kp**:
- \( K_p \) is the equilibrium constant, which is a constant value at a given temperature when the system is at equilibrium.
- Since the forward reaction is favored and products are being formed, \( Q_p \) must be less than \( K_p \) because equilibrium has not been reached yet.

7. **Conclusion**:
Since the concentration of products is increasing and the concentration of reactants is decreasing, we can conclude that:
\[ Q_p < K_p \]
Therefore, the correct answer is:
**(C) \( Q_p < K_p \)**.