Each question given below contains STATEMENT -1 (Assertion) and STATEMENT -2 (Reason). It has four choice (a), (b), ( c ) and (d) out of which ONLY ONE is correct . Choose the correct option as under :
Statement -1 `K_(p)` is always greater than `K_(c)`
Statement -2 . The reactions in the gaseous phase are usually faster than the reactions in the liquid phase.

Explanation

To solve the question regarding the correctness of the statements provided, we need to analyze both Statement 1 (Assertion) and Statement 2 (Reason) carefully.

### Step 1: Analyze Statement 1
Statement 1: **Kp is always greater than Kc.**

- Kp (equilibrium constant for gaseous reactions) and Kc (equilibrium constant for reactions in terms of concentration) are related by the equation:

\[ Kp = Kc \times (RT)^{\Delta n_g} \]

where:
- R = universal gas constant,
- T = temperature in Kelvin,
- \(\Delta n_g\) = change in the number of moles of gas (moles of gaseous products - moles of gaseous reactants).

- From this equation, we can see that Kp can be greater than, equal to, or less than Kc depending on the value of \(\Delta n_g\) and the temperature (T). Therefore, it is incorrect to state that Kp is always greater than Kc.

### Conclusion for Statement 1:
- **Statement 1 is false.**

### Step 2: Analyze Statement 2
Statement 2: **The reactions in the gaseous phase are usually faster than the reactions in the liquid phase.**

- In general, reactions in the gaseous phase tend to occur faster than those in the liquid phase. This is primarily due to the lower intermolecular forces in gases compared to liquids, allowing gas molecules to collide more freely and frequently, thus facilitating faster reactions.

### Conclusion for Statement 2:
- **Statement 2 is true.**

### Final Conclusion:
- Since Statement 1 is false and Statement 2 is true, the correct answer to the question is **(d)**.