11.What is the difference between Ideal gases and Real gases?
-

Explanation:

They are the gases that conform to gas laws under all conditions of temperature and pressure. They are the gases that conform precisely to the assumptions of kinetic theory. ideal gases according to the kinetic theory assumptions could have no significant volume and there is no attractive or repulsive forces between its particles. there is no gas for which these assumptions are true; an ideal gas does not exist.  However, under many coditions of temperature and pressure real gases behave much like ideal gases. Real gases have volume and there are attractions between their particles. Because of these attractions, real gases can be solidified or condensed when compressed or cooled e.g. water vapor when cooled below 100 degrees celsius at standard atmospheric pressure  can be condensed into liquid. other real gases behave like that but sometimes more pressure and less temperature is required.

Assumptions of kinetic theory:

the volume of a single particle in gas is small compared to the overall volume of the gas.under pressure, the particles are compressed and come closer together.there are no attractice or repulsive forces between its particles so it can move freelyit expand to take the shape and size of the containerthe particles of the gas move in straight path until they collide with the wall of the container or with each otherthe motion of the particles is rapid, random and constantthe distance between the particles of gas is more than that between solids and liquids

1. Subtract 4 from both sides
v - 4 = 2t
2. Divide both sides by 2
v - 4/2 = t
3. Switch sides
t = v - 4/2