A gas behave most like an Ideal gas under conditions of

Options

A. High pressure and low temperature
B. High temperature and high pressure
C. low pressure and high temperature
D. Low pressure and low temperature

Explanation

To determine the conditions under which a gas behaves most like an ideal gas, we can follow these steps:

### Step 1: Understand the Characteristics of Ideal Gases
Ideal gases are theoretical gases that perfectly follow the gas laws under all conditions. They have no intermolecular forces and occupy no volume.

### Step 2: Identify Conditions for Real Gases
Real gases deviate from ideal behavior due to intermolecular forces and the volume occupied by gas molecules. The behavior of real gases approaches that of ideal gases under certain conditions.

### Step 3: Recognize High Temperature and Low Pressure
Real gases behave most like ideal gases at high temperatures and low pressures.
- **High Temperature**: At high temperatures, the kinetic energy of gas molecules increases, which helps to overcome intermolecular forces. This means that the gas molecules are moving fast enough that they do not interact significantly with one another.
- **Low Pressure**: At low pressures, the volume of the gas molecules becomes negligible compared to the volume of the container. This minimizes the effects of the finite size of the gas molecules.

### Step 4: Conclusion
Thus, the conditions under which a gas behaves most like an ideal gas are high temperature and low pressure.

### Final Answer
A gas behaves most like an ideal gas under conditions of **high temperature and low pressure**.

---