Statement-1. In the reaction, `N_(2)+3" H"_(2)to 2" NH"_(3)`, the rate of reaction is different in terms of `N_(2), H_(2)` and `NH_(3)`.
Statement-2. Rate of disappearance of `N_(2)` and `H_(2)` and rate of formation of `NH_(3)` are not equal to each other.

Options

A. Statement-1 is True, Statement-2 is True , Statement-1 is a correct explanation of Statement-1.
B. Statement-1 is True, Statement-2 is True , Statement-2 is NOT the correct explanation of Statement-1.
C. Statement-1 is True, Statement-2 is False.
D. Statement-1 is False, Statement-2 is True.

Explanation

To analyze the statements given in the question, we will break down the reaction and the rates of disappearance and formation of the reactants and products.

### Step-by-Step Solution:

1. **Understanding the Reaction:**
The reaction given is:
\[ N_2 + 3 H_2 \rightarrow 2 NH_3 \]
This means that one mole of nitrogen reacts with three moles of hydrogen to produce two moles of ammonia.

2. **Writing the Rate Expressions:**
The rate of a reaction can be expressed in terms of the change in concentration of the reactants and products over time. For this reaction, we can write:
\[ \text{Rate} = -\frac{d[N_2]}{dt} = -\frac{1}{3}\frac{d[H_2]}{dt} = \frac{1}{2}\frac{d[NH_3]}{dt} \]

3. **Analyzing the Rate of Disappearance and Formation:**
From the rate expressions:
- The rate of disappearance of \(N_2\) is given by \(-\frac{d[N_2]}{dt}\).
- The rate of disappearance of \(H_2\) is given by \(-\frac{1}{3}\frac{d[H_2]}{dt}\).
- The rate of formation of \(NH_3\) is given by \(\frac{1}{2}\frac{d[NH_3]}{dt}\).

4. **Comparing the Rates:**
To compare these rates, we can express them in terms of a common rate (let's denote it as \(R\)):
- For \(N_2\): \(R = -\frac{d[N_2]}{dt}\)
- For \(H_2\): \(R = -3\frac{d[H_2]}{dt}\)
- For \(NH_3\): \(R = 2\frac{d[NH_3]}{dt}\)

This shows that the rates are not equal in terms of their absolute values because they are related by their stoichiometric coefficients.

5. **Evaluating the Statements:**
- **Statement 1:** "The rate of reaction is different in terms of \(N_2\), \(H_2\), and \(NH_3\)." This statement is **true** because the rates of disappearance and formation are indeed different when expressed in terms of their stoichiometric coefficients.
- **Statement 2:** "Rate of disappearance of \(N_2\) and \(H_2\) and rate of formation of \(NH_3\) are not equal to each other." This statement is also **true** because, as shown, the rates are related by their stoichiometric coefficients and are not equal in absolute terms.

6. **Conclusion:**
Both statements are true, but the first statement can be misleading if not understood correctly in terms of stoichiometry. Therefore, the correct interpretation is that while the rates are related, they are expressed differently based on the stoichiometric coefficients.

### Final Answer:
- **Statement 1:** True
- **Statement 2:** True