The temperature at which real gases obey the ideal gas laws over a wide range of low pressure is called:
(a)Critical temperature
(b)Inversion temperature
(c)Boyle temperature
(d)Reduced temperature

Options

A. Critical temperature
B. Inversion temperature
C. Boyle temperature
D. Reduced temperature

Explanation

To solve the question regarding the temperature at which real gases obey the ideal gas laws over a wide range of low pressure, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Ideal Gas Law**:
The ideal gas law is given by the equation \( PV = nRT \), where:
- \( P \) = pressure
- \( V \) = volume
- \( n \) = number of moles
- \( R \) = ideal gas constant
- \( T \) = temperature

2. **Real Gases vs Ideal Gases**:
Real gases deviate from ideal behavior under certain conditions, especially at high pressures and low temperatures. However, at low pressures and certain temperatures, real gases can behave more like ideal gases.

3. **Identifying Boyle's Temperature**:
Boyle's temperature is defined as the temperature at which a real gas behaves ideally at low pressures. At this temperature, the compressibility factor \( Z \) (which is defined as \( Z = \frac{PV}{nRT} \)) approaches 1, indicating that the gas follows the ideal gas law.

4. **Conclusion**:
Based on the definitions and understanding of gas behavior, the temperature at which real gases obey the ideal gas laws over a wide range of low pressure is known as Boyle's temperature.

5. **Final Answer**:
Therefore, the correct answer is (c) Boyle temperature.