Which of the following statements would correctly explain the non-ideal behavior of a gas based on the Kinetic Molecular Theory (KMT)?

• A. At high temperatures the attractive forces between molecules becomes negligible.
• B. At high pressure the volume of gas molecules become significant.
• C. An increase or decrease in the moles of gas causes the gas constant value to change.

Answer: (B)

Verified step by step guidance

1. Begin by understanding the Kinetic Molecular Theory (KMT), which assumes that gas particles are in constant random motion and that they occupy negligible volume compared to the container they are in.
2. Recognize that KMT assumes no intermolecular forces between gas particles, meaning they do not attract or repel each other under ideal conditions.
3. Identify the conditions under which gases deviate from ideal behavior: high pressure and low temperature. At high pressure, the volume occupied by gas molecules becomes significant compared to the container volume.
4. Understand that at high pressure, the assumption that gas particles have negligible volume is no longer valid, leading to non-ideal behavior as the particles occupy a larger fraction of the container's volume.
5. Note that the gas constant value (R) does not change with the number of moles of gas; it is a constant in the ideal gas law equation, which is another reason why the statement about moles affecting the gas constant is incorrect.