When considering two different types of ideal gases, it is important to note that when the two substances exist as different, yet equal, molar samples, they will exhibit significantly different behaviors. This includes differences in pressure, temperature, volume, and number of moles. While the underlying laws of ideal gases remain the same, there are significant differences in the behavior of different gases when contained in the same volume.
For example, when equimolar samples of two different ideal gases are placed in a closed container, the pressure of each gas will be different. This phenomenon occurs because the individual molecules of different ideal gases have different sizes, as well as different masses. The heavier the molecule, the larger the force applied to the container walls, resulting in a higher pressure.
At normal room temperature and pressure, the relationship between the temperature and pressure of different ideal gases remains the same. However, when the temperature and pressure are altered, the relationship between the two is no longer uniform. In fact, when either the temperature or pressure is changed, the behavior of one gas may be different from the other.
In addition, the volume of the container also affects the behavior of different ideal gases. As the container volume increases, the pressure on each gas increases, ultimately resulting in a decrease in the number of moles of each gas. This effect is known as the gas law, and it is one of the most important factors to consider when working with different ideal gases.
A single sample of an ideal gas is usually composed of a single type of molecule, thus it is capable of exhibiting only one type of behavior. However, when two or more different ideal gases are mixed together, their behavior can vary significantly. This is because each gas molecule is different and has its own set of properties. As a result, when two different ideal gases are placed together, they will typically experience a wide range of interactions that will be different from what could be expected with a single gas.
The behavior of different ideal gases in equimolar samples is highly dependent on the underlying laws of thermodynamics and the specific properties of each gas. As such, it is important to understand how each gas behaves and how they interact with each other before attempting to mix different ideal gases together.