A chemist is studying the properties of a gas under various conditions. He observes that when the gas is at room temperature and low pressure, it behaves as an ideal gas. When the gas is cooled to 10 kelvin (–263ºC) and is placed under high pressure, however, it deviates significantly from an ideal gas. There are multiple reasons for this phenomenon. Check all of the correct reasons below.
The ideal gas model assumes that gas particles experience no intermolecular attractions and these forces cause the gas to deviate from ideal behavior.
At very low temperatures, gas particles move slowly.
At very high pressures, gas particles are very close together.
Gases placed under high pressure will undergo deposition, changing from a gas to a solid.
The ideal gas model assumes that gas particles experience no intermolecular attractions and these forces cause the gas to deviate from ideal behavior.
At very high pressures, gas particles are very close together.