Final answer:
Entropy relates to the disorder or randomness of a system, with gases typically having the highest entropy, followed by liquids, and then solids. Higher temperatures and more complex molecules also contribute to greater entropy. Hence, H₂O(l) would be expected to have greater entropy than H₂O(s) but less than H₂O(g).
Step-by-step explanation:
The question revolves around predicting which sample would have the greatest entropy. Entropy is a measure of the randomness or disorder of a system. In the context of chemistry, it helps us understand how different states of matter and molecular complexity affect the distribution of energy within a system. When comparing different samples or states of matter, a general rule is that gases have higher entropy than liquids and solids, and among solids and liquids, those that are at higher temperatures usually have higher entropy because the molecules have more energy and can occupy more states.
When considering H₂O(l), or other substances in various phases and conditions, entropy tends to increase from solid to liquid to gas due to the increased freedom of motion for molecules. Higher temperatures also contribute to increased entropy, as they imply greater molecular motion. Additionally, more complex molecules with more atoms have higher entropy because they have more possible microstates. Given this information, we can deduce that the liquid phase of a substance generally has higher entropy than the solid phase, and gases have the highest entropy among the states of matter due to their freedom of motion.