what r ideal gases and non-ideal gases?
what r ideal gases and non-ideal gases?
An ideal gas is a hypothetical gas consisting of particles that could be atoms or molecules such that the particles that constitute the gas collide with each other in a perfectly elastic manner. Also the particles should not have any attractive forces between each other. If the gas can be pictured as one that is made up of perfectly hard spheres with no inter particulate attraction it is called an ideal gas. Internal energy in an ideal gas is purely kinetic, and a change in temperature is accompanied by a proportional change in energy. An ideal follows al gas laws (Boyle's law, Charles law, etc.) at all temperature and pressure conditions.
This can be expressed by the relation PV= nRT perfectly. Here P is the pressure, V is the volume, n is the number of moles, R is the universal gas constant and T is the temperature. Gases around us are not ideal gases, so the ideal gas law is a close fit but does not exactly express the properties of gases.
Non ideal gases on the other hand are real gases that are found around us. They do not follow gas laws at all conditions of temperature and pressure. Also the collision between the particles of a non ideal gas are inelastic.
Note that real gases behave as ideal gases at high temperature and low pressure.
An ideal gas is a hypothetical gas consisting of particles that could be atoms or molecules such that the particles that constitute the gas collide with each other in a perfectly elastic manner. Also the particles should not have any attractive forces between each other. If the gas can be pictured as one that is made up of perfectly hard spheres with no inter particulate attraction it is called an ideal gas. Internal energy in an ideal gas is purely kinetic, and a change in temperature is accompanied by a proportional change in energy. An ideal follows al gas laws (Boyle's law, Charles law, etc.) at all temperature and pressure conditions.
This can be expressed by the relation PV= nRT perfectly. Here P is the pressure, V is the volume, n is the number of moles, R is the universal gas constant and T is the temperature. Gases around us are not ideal gases, so the ideal gas law is a close fit but does not exactly express the properties of gases.
Non ideal gases on the other hand are real gases that are found around us. They do not follow gas laws at all conditions of temperature and pressure. Also the collision between the particles of a non ideal gas are inelastic.
Note that real gases behave as ideal gases at high temperature and low pressure.
