Boyle's law for gases is:
true for all gases
only accurate at room temperature
just a model and therefore accurate for no real gas
accurate for most gases in most temperature ranges
a good example of a "law" that is now found to be incorrect

Just a model and therefore accurate for no real gas because ideal gas laws were proposed by assuming that 1. The gas consists of large number of molecules which moves randomly and obey newton's laws of motion. 2. The volume of molecules is negligibly small compared to the volume occupied by the gas and no force act on the molecules except during the elastic collision. No real gas obey this properties, except only at high temperatures and low pressures, hence it is accurate for no real gases( ideal gases). 

J. All of these

Explanation:

I hope it helps.