Why do real gases not behave exactly like ideal gases?

An ideal gas is a hypothetical gas consisting of identical particles of negligible volume, with no intermolecular forces. Also the atoms or molecules of the gas undergo perfectly elastic collisions with the walls of the container and each other. Real gases do not exhibit these exact properties.

because the particals will not move the same as real gases

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.