Which of the following statements is/are correct with respect to behaviour of real gas. 

Options

A. a) For every vander Waal gas at critical condition, attractive force will be dominant
B. b) The liquid and gaseous state can be distinguished only if the temperature is below the gas's critical temperature.
C. c) At very high pressures, real gases occupy greater volume as compared to ideal gas having same moles at same temperature and exerting same pressure.
D. d) For a real gas the 'y' intercept of `(PV_(m))/T` vs curve where 'P' represents pressure (in atm), `V_(m)` represents molar volume and 'T' represents temperature in kelvin is equal to 0.0821 atm-litre/mol Kelvin

Answer

To determine which statements regarding the behavior of real gases are correct, we will analyze each statement one by one.

### Step-by-Step Solution:

**Step 1: Analyze Statement A**
- **Statement A**: "For every Van der Waals gas at critical condition, attractive force will be dominant."
- **Analysis**: At the critical point of a Van der Waals gas, the attractive forces between molecules become significant due to the thermal motion of the gas molecules. Therefore, this statement is correct.

**Conclusion for Step 1**: Statement A is correct.

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**Step 2: Analyze Statement B**
- **Statement B**: "The liquid and gaseous state can be distinguished only if the temperature is below the gaseous critical temperature."
- **Analysis**: Liquid and gas can be distinguished not only when the temperature is below the critical temperature but also when it is above the critical temperature. Thus, this statement is misleading as it implies exclusivity. Therefore, this statement is incorrect.

**Conclusion for Step 2**: Statement B is incorrect.

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**Step 3: Analyze Statement C**
- **Statement C**: "At very high pressure, real gas occupies greater volume as compared to ideal gas having the same moles at the same temperature and exerting the same pressure."
- **Analysis**: At high pressures, real gases deviate from ideal behavior. Due to intermolecular forces and the finite volume of gas molecules, real gases occupy a greater volume than predicted by the ideal gas law. Therefore, this statement is correct.

**Conclusion for Step 3**: Statement C is correct.

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**Step 4: Analyze Statement D**
- **Statement D**: "For a real gas, the intercept of PVM/T versus T curve is equal to 0.0821 ATM litre per mole Kelvin."
- **Analysis**: The equation of state for an ideal gas is PV = nRT, which can be rearranged to PVM/T = nR. The constant R is indeed 0.0821 ATM litre per mole Kelvin, which is the ideal gas constant. Therefore, this statement is correct.

**Conclusion for Step 4**: Statement D is correct.

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### Final Conclusion:
Based on the analysis:
- Statement A: Correct
- Statement B: Incorrect
- Statement C: Correct
- Statement D: Correct

Thus, the correct statements regarding the behavior of real gases are A, C, and D.