Which of the following choices match(es) with hydrogen gas at 200 atm and 273 K?

Options

A. `Zne1`
B. Attractive forces are dominant
C. PV = nRT
D. P(V - nb) = nRT

Answer

To solve the question regarding the behavior of hydrogen gas at 200 atm and 273 K, we need to analyze the conditions provided and apply the principles of gas behavior under high pressure and low temperature.

### Step-by-Step Solution:

1. **Identify the Conditions**:
- Pressure (P) = 200 atm (high pressure)
- Temperature (T) = 273 K (low temperature, equivalent to 0°C)

2. **Understand Gas Behavior**:
- At high pressures, gases tend to deviate from ideal gas behavior. This is because the volume occupied by the gas molecules becomes significant compared to the volume of the container, and intermolecular forces become important.

3. **Real Gas Behavior**:
- Under these conditions (high pressure and low temperature), hydrogen gas will behave more like a real gas rather than an ideal gas. This means that the compressibility factor (Z) will not equal 1, which is a characteristic of ideal gases.

4. **Use the Van der Waals Equation**:
- The Van der Waals equation for real gases is given by:
\[ \left(P + \frac{a n^2}{V^2}\right)(V - nb) = nRT \]
- Here, \(a\) and \(b\) are constants that account for the intermolecular forces and the volume occupied by the gas molecules, respectively.

5. **Analyze the Options**:
- Since the question asks which choices match with hydrogen gas under the given conditions, we need to look for options that reflect the real gas behavior (Z ≠ 1) and the implications of high pressure and low temperature.

6. **Conclusion**:
- The options that reflect the behavior of hydrogen gas at 200 atm and 273 K would be those that indicate the gas is behaving as a real gas, which includes increased repulsive forces and deviations from ideal gas laws.

### Final Answer:
The correct choices that match with hydrogen gas at 200 atm and 273 K would be the options that indicate real gas behavior, specifically the first and fourth options.