Real gases are not ideal gases. Explain why this is so in terms of intermolecular forces, and then describe (and justify) what conditions with regard to temperature and pressure will bring a real gas close to behaving like an ideal gas.

An ideal gas is a hypothetical gas that follows the ideal gas law, PV=nRT, where P is pressure, V is volume, n is the number of moles of the gas, R is the ideal gas constant, and T is temperature in Kelvin. In an ideal gas, there are no intermolecular forces, the particles are assumed to have no volume, and they move in random motion. On the other hand, real gases deviate from the ideal gas behavior due to the presence of intermolecular forces and the actual volume of the gas particles.

In a real gas, the particles have intermolecular forces (attractive and repulsive forces) that can affect their behavior. The attractive forces between molecules cause them to be attracted to each other and this lowers the pressure of the gas compared to an ideal gas under the same conditions. The repulsive forces between molecules cause them to be repelled from one another, thus making the volume they occupy even larger than that predicted by the ideal gas law.

There are certain conditions under which a real gas can behave like an ideal gas. These conditions relate to temperature and pressure. 1. High temperature: At high temperatures, the kinetic energy of gas particles increases, which allows the particles to overcome the attractive forces between them. Hence, the gas particles move more freely and exhibit behavior similar to an ideal gas. Also, at high temperatures, the repulsive forces will be less significant, as particles will have a higher tendency to move away from each other. 2. Low pressure: At low pressure, the gas particles are far apart from each other, reducing the influence of intermolecular forces. The attractive forces will be less significant because the particles are not close enough for these forces to be effective. Moreover, the repulsive forces will also be less significant, as particles will have enough space to move without coming into close contact with each other. This allows the gas to expand more freely and approach ideal gas behavior. Under these conditions, real gases will exhibit behavior close to an ideal gas, since the intermolecular forces become much less significant when compared to the kinetic energy of the particles and the separation between them.