Question

Under what conditions will a gas be least likely to exhibit the ideal gas properties predicted by the ideal gas law?

A) High pressures and high temperature, because particles are forced closer together with higher kinetic energy, so intermolecular forces of attraction increase
B) High pressure and low temperature, because particles are forced closer together and moving slower, so intermolecular forces of attraction increase
C) Low pressure and high temperature, because particles are spread farther apart and faster moving, so the volume of the particles is more significant
D) Low pressure and low temperature, because particles are spread farther apart with lower kinetic energy, so the volume of the particles is more significant
a) Option A
b) Option B
c) Option C
d) Option D

Answer 1

The correct answer is option B. A gas will be least likely to exhibit ideal gas properties at high pressures and low temperatures because the molecules are forced closer together and have lower kinetic energy, leading to stronger intermolecular forces of attraction. This violates the assumption of negligible volume in the ideal gas law.

Step-by-step explanation:

A gas will be least likely to exhibit the ideal gas properties predicted by the ideal gas law at high pressures and low temperatures (Option B) because the molecules are forced closer together and have lower kinetic energy, leading to stronger intermolecular forces of attraction.

At high pressures, the volume of the gas molecules themselves becomes appreciable compared to the total volume occupied by the gas, violating the assumption of negligible volume in the ideal gas law. Additionally, at low temperatures, the decrease in kinetic energy of the molecules makes them less effective in overcoming the attractive forces between them.