For non-zero value of force of attraction between gas molecular at large volume, gas equation will be :
(a)`PV=nRT-(n^(2)a)/(V)`
(b)`PV=nRT+nbP`
(c)`P=(nRT)/(V-b)`
(d)`PV=nRT`

Options

A. `PV=nRT-(n^(2)a)/(V)`
B. `PV=nRT+nbP`
C. `P=(nRT)/(V-b)`
D. `PV=nRT`

Explanation

To solve the question regarding the gas equation for a non-zero value of force of attraction between gas molecules at large volume, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Context**: The question refers to the behavior of real gases, particularly when there is a non-zero force of attraction between gas molecules. This means we need to consider the Van der Waals equation for real gases.

2. **Recall the Van der Waals Equation**: The Van der Waals equation for real gases is given by:
\[ \left(P + \frac{a n^2}{V^2}\right)(V - nb) = nRT \]
where:
- \(P\) = pressure of the gas
- \(V\) = volume of the gas
- \(n\) = number of moles of the gas
- \(R\) = universal gas constant
- \(T\) = temperature
- \(a\) = measure of the attraction between particles
- \(b\) = volume occupied by one mole of the gas particles

3. **Consider Large Volume**: At large volumes, the effect of intermolecular forces becomes negligible. Thus, the term \(\frac{a n^2}{V^2}\) can be considered small and can be neglected.

4. **Simplify the Equation**: Neglecting the attraction term, the equation simplifies to:
\[ P(V - nb) = nRT \]

5. **Rearranging the Equation**: Expanding this gives:
\[ PV - Pnb = nRT \]
Rearranging leads to:
\[ PV = nRT + Pnb \]

6. **Identify the Correct Option**: The rearranged equation \(PV = nRT + Pnb\) matches with option (b) from the question:
\[ PV = nRT + nbP \]

### Conclusion:
The correct answer is option (b):
\[ PV = nRT + nbP \]