Graph depicting correct behaviour of ideal gas and `H_(2)` gas will be (neglect a):

Answer

To solve the question regarding the graph depicting the correct behavior of ideal gas and \( H_2 \) gas, we will analyze the behavior of both gases based on the ideal gas law and the modifications for real gases.

### Step-by-Step Solution:

1. **Understanding Ideal Gas Behavior**:
- The ideal gas law is given by the equation:
\[ PV = nRT \]
- This equation assumes that the gas behaves ideally, meaning there are no intermolecular forces and the volume of the gas particles themselves is negligible.

2. **Understanding Real Gas Behavior**:
- For real gases, we can use the Van der Waals equation, which accounts for the volume occupied by gas molecules and the intermolecular forces:
\[ \left(P + \frac{a n^2}{V^2}\right)(V - nB) = nRT \]
- Here, \( a \) and \( b \) are constants specific to each gas. However, in this case, we are instructed to neglect the constant \( a \) for \( H_2 \).

3. **Simplifying the Van der Waals Equation for \( H_2 \)**:
- Neglecting the \( a \) term, the equation simplifies to:
\[ P(V - nB) = nRT \]
- Rearranging gives:
\[ PV - nBP = nRT \]
- This can be rewritten as:
\[ PV = nRT + nBP \]

4. **Comparing Ideal Gas and Real Gas**:
- From the above equation, we can see that for any given values of \( P \) and \( V \), the term \( nBP \) is added to the ideal gas equation.
- This implies that the product \( PV \) for the real gas (in this case, \( H_2 \)) will be greater than that for the ideal gas:
\[ PV_{\text{real}} > PV_{\text{ideal}} \]

5. **Graphical Representation**:
- On a graph where the x-axis represents the volume (V) and the y-axis represents the pressure (P), the curve for the ideal gas will lie below the curve for the real gas \( H_2 \) at the same conditions of temperature and number of moles.
- Therefore, the correct graph will show the ideal gas behavior as a lower curve compared to the \( H_2 \) gas behavior.

6. **Conclusion**:
- The correct answer to the question is option A, which depicts the behavior of \( H_2 \) gas being higher than that of an ideal gas for the same conditions.