At room temperature, 20° C, water (H2O) is a liquid and oxygen (O2) is a gas. Based on kinetic molecular theory, which answer best explains the states of the two fluids?

a The particles in the liquid have greater kinetic energy than the particles in the gas.
b The particles in both substances are able to flow because of weak intermolecular forces.
c The particles in both substances are able to fill any container because both have indefinite shape and indefinite volume.
d Water molecules have a lower boiling temperature than oxygen molecules, so at room temperature they exist as a liquid rather than a gas.

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The correct answer is d: Water molecules have a lower boiling temperature than oxygen molecules, so at room temperature they exist as a liquid rather than a gas.

To understand why this is the correct answer, let's break it down based on the concepts of kinetic molecular theory.

Kinetic molecular theory explains that matter is made up of particles (atoms or molecules) that are in constant motion. The state of a substance (solid, liquid, or gas) is determined by the average kinetic energy of its particles.

In the case of water and oxygen, both substances are at room temperature, which is 20° C. At this temperature, water exists as a liquid while oxygen exists as a gas.

The reason for this difference lies in the intermolecular forces between the particles of each substance. Water molecules have stronger intermolecular forces compared to oxygen molecules. These forces hold the water molecules closer together, making it more difficult for them to escape into the gas phase.

Oxygen molecules, on the other hand, have weaker intermolecular forces, allowing them to move more freely and easily escape into the gas phase. This is why oxygen is a gas at room temperature.

So, the correct answer d explains that water molecules have a lower boiling temperature than oxygen molecules, which is why water exists as a liquid at room temperature while oxygen exists as a gas.

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