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The selected answer highlights that butane does not vaporize adequately below 32°F, which relates to the physical properties of butane as a hydrocarbon. Butane has a boiling point of approximately 31°F (-0.5°C) at standard atmospheric pressure. Below this temperature, butane exists primarily in its liquid state, meaning that there isn’t enough thermal energy for the butane molecules to overcome intermolecular forces and enter the vapor phase efficiently.

At temperatures above its boiling point, however, butane readily vaporizes, so the correct understanding of its behavior is that insufficient thermal energy at lower temperatures halts adequate vaporization. Therefore, the dynamics of temperature in regard to its phase change play a critical role; as the temperature rises and surpasses the boiling point, butane can vaporize effectively. This comprehension aligns with how temperature influences physical changes in substances based on their boiling points.