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's A.
Thank You.
Yes the answer is A.
Answers for Connexus Honors Chemistry.
Unit 1 Lesson 8 Ideal Gases
1-A Number of moles.
2-C PV=nRT.
3-A It is much greater.
4-A Condensed
Trust me 100%
To determine how the volume of a real gas compares to an ideal gas under high pressures, we can refer to the behavior of gases based on the principles of the Ideal Gas Law.
The Ideal Gas Law equation is given by: PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature.
Under high pressures, the behavior of real gases tends to deviate from the behavior predicted by the ideal gas law. Real gases exhibit intermolecular forces and occupy space, unlike the assumption made for ideal gases.
In general, at high pressures, real gases tend to occupy more volume compared to ideal gases under the same conditions. This is because the intermolecular forces between the gas molecules become significant, resulting in the expansion of the gas volume.
Therefore, the correct answer is B.) It is much less. The volume of a real gas is generally lower than the volume of an ideal gas at pressures greater than 60,000 kPa under the same conditions.
Remember, when dealing with questions like this, it's important to have a good understanding of the gas laws, including the Ideal Gas Law equation, and the behavior of real gases under different conditions.