A real gas can be approximated to an idcal gas at

Options

A. low density
B. high pressure
C. high density
D. low temperature

Answer

To determine the conditions under which a real gas can be approximated as an ideal gas, we can analyze the behavior of gases under different conditions. Here’s a step-by-step solution:

### Step 1: Understand the Ideal Gas Law
The ideal gas law is given by the equation:
\[ PV = nRT \]
where:
- \( P \) = pressure
- \( V \) = volume
- \( n \) = number of moles of gas
- \( R \) = universal gas constant
- \( T \) = temperature

### Step 2: Identify Conditions for Ideal Behavior
Real gases deviate from ideal behavior under certain conditions. Generally, a real gas behaves more like an ideal gas when:
1. The pressure is low.
2. The temperature is high.
3. The density is low.

### Step 3: Analyze the Given Options
The options provided are:
- Low density
- High pressure
- High density
- Low temperature

### Step 4: Evaluate Each Option
- **Low Density**: This condition allows gas molecules to be far apart, minimizing intermolecular forces, which makes the gas behave more ideally. **(Correct)**
- **High Pressure**: At high pressure, gas molecules are closer together, leading to significant intermolecular forces, causing deviations from ideal behavior. **(Incorrect)**
- **High Density**: Similar to high pressure, high density implies that molecules are close together, which leads to non-ideal behavior. **(Incorrect)**
- **Low Temperature**: At low temperatures, gas molecules have lower kinetic energy, which increases the effect of intermolecular forces, leading to deviations from ideal behavior. **(Incorrect)**

### Step 5: Conclusion
From the analysis, the only condition under which a real gas can be approximated to an ideal gas is at **low density**.

### Final Answer
A real gas can be approximated to an ideal gas at **low density**.

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