is it right that ideal gas only obey the boyles law under high temp and low pressure?
"Ideal" means PV = n R T
If it does not obey the simple gas laws, it is not "ideal".
so how about this question?
Which of the following desceriptions about ideal gas is/are correct?
1)An ideal gas obeys Boyle's law only under high temp and low pressure
2)the molecules of an ideal gas have no size
3)the internal energy of an ideal gas consists of kinetic energy only
A.1)only B.3)only
C.1)&2) D.2)&3)
THE ANS IS D but not 1,2,3 are correct,why?
No, it is not accurate to say that ideal gases only obey Boyle's law under high temperature and low pressure. In reality, ideal gases follow Boyle's law at all temperatures and pressures, as long as other conditions remain constant.
Boyle's law states that for a given amount of gas at a constant temperature, the pressure and volume of the gas are inversely proportional. Mathematically, this can be expressed as P ∝ 1/V, where P is the pressure and V is the volume.
Under high temperatures and low pressures, gases tend to behave more ideally, meaning they approximate ideal gas behavior more closely. However, even under different temperature and pressure conditions, ideal gases still follow Boyle's law as long as the temperature and amount of gas do not change.
To verify this, you can perform experiments or use mathematical calculations to measure the pressure and volume of a gas sample under different conditions while ensuring that the temperature and amount of gas remain constant. By observing the resulting data, you will see that Boyle's law holds true for ideal gases across a wide range of temperatures and pressures.