At pressures greater than 60,000 kPa, how does the volume of a real gas compare with the volume of an ideal gas under the same conditions?
A.)It is much greater.
B.)It is much less.
C.)There is no difference.
D.)It depends on the type of gas.
I think it is A.
Thank You.
Why not pick n(mols) and a convenient T (say 300 K) and a pressure (say 70,000 kPa) and calculate volume using the ideal gas law versus the van der waals equation for some gas (I wouldn't use H2 as but something like CH4 or CO2). Compare.
To determine how the volume of a real gas compares to that of an ideal gas at pressures greater than 60,000 kPa, we need to understand the behavior of gases under such conditions.
An ideal gas is a theoretical concept that follows the gas laws perfectly, including Boyle's law, Charles's law, and Avogadro's law. According to these laws, at constant temperature and pressure, the volume of an ideal gas is inversely proportional to its pressure. Therefore, as pressure increases, the volume of an ideal gas decreases.
However, real gases deviate from ideal gas behavior, especially at higher pressures and lower temperatures. At high pressures, the volume of a real gas is generally smaller than that predicted by the ideal gas law. This is because real gases occupy a finite volume and have intermolecular forces and molecular sizes that can affect their behavior.
Therefore, the correct answer is B.) It is much less. The volume of a real gas tends to be smaller than the volume of an ideal gas under the same conditions at pressures greater than 60,000 kPa.
Remember, it is always important to consider the properties and behavior of gases, as well as the gas laws, when comparing real and ideal gases.