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.

At high pressure the volume of gas molecules become significant.

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.

Here in this practice question it says, which of the following statements will correctly explain the non ideal behavior of a gas based on the kinetic molecular theory? Alright. So ideal behavior, postulate 1 says that an ideal gas has no real volume. Its volume is so low and insignificant. It's less than 0.01% of the total volume in the container. The second postulate says that an ideal gas, as the temperature increases its velocity increases. And then postulate 3 says that an ideal gas has completely elastic collisions or it has no attractive or repulsive forces. So here, a, at high temperatures the attractive forces between molecules becomes negligible. Negligible meaning non important. Well, that is exactly what an ideal gas wants. It doesn't want attractive forces. It wants them to be insignificant. So here, this is talking about ideal gas behavior, not non ideal gas behavior. At high pressures, the volume of a gas becomes significant. Alright. So remember, postulate 1 says that the volume of a gas molecule is insignificant or negligible because it's less than 0.01%. B is saying the exact opposite, so it's talking about non ideal behavior for gas. So this would be our answer. C, an increase or decrease in the moles of a gas, causes the gas constant value to change. Alright. So remember our gas constant r, it doesn't change, based on the moles of a gas. Now the number for for r can change based on units. Okay? But this statement is just not true. It has nothing to do with non ideal or ideal gas behavior. So the best answer here out of the three choices would have to be option b. It goes against the whole idea of the volume of an ideal gas being insignificant or negligible.