is that right ideal gas only obey the boyles law under high temp and low pressure?
No, that statement is not entirely correct.
An ideal gas obeys Boyle's Law at any temperature and pressure. Boyle's Law states that, at constant temperature, the volume of a given amount of gas is inversely proportional to its pressure. Mathematically, this relationship can be expressed as:
P₁V₁ = P₂V₂,
where P₁ and P₂ are the initial and final pressures of the gas, and V₁ and V₂ are the initial and final volumes, respectively.
However, it is important to note that the behavior of a real gas may deviate from the predictions of Boyle's Law at high pressures and/or low temperatures due to various factors, such as intermolecular interactions and molecular volume. These deviations can be more pronounced for real gases as compared to ideal gases. In such cases, more sophisticated equations of state, such as the Van der Waals equation, can provide a better description of the behavior of the gas.