At 25 °C gallium is a solid with a density of 5.91 g/cm^3

Question

At 25 °C gallium is a solid with a density of 5.91 g/cm³. Its melting point, 29.8 °C, is low enough that you can melt it by holding it in your hand. The density of liquid gallium just above the melting point is 6.1 g/cm³. Based on this information, what unusual feature would you expect to find in the phase diagram of gallium?

Accepted Answer

Step 1: Understand the problem. The problem provides information about the density of gallium in its solid and liquid states. The density of solid gallium is less than the density of liquid gallium.. Step 2: Recall the general trend in phase diagrams. Typically, the solid phase of a substance is denser than its liquid phase. This is because particles in a solid are usually packed more closely together than in a liquid.. Step 3: Compare the general trend with the given information. In the case of gallium, the liquid phase is denser than the solid phase. This is contrary to the general trend.. Step 4: Predict the unusual feature in the phase diagram. Given that the liquid phase of gallium is denser than its solid phase, we would expect the phase diagram of gallium to show the solid-liquid boundary sloping to the right with increasing pressure. This is unusual because for most substances, the solid-liquid boundary in a phase diagram slopes to the left with increasing pressure.. Step 5: Understand the reason behind this unusual feature. The slope of the solid-liquid boundary in a phase diagram is determined by the relative densities of the solid and liquid phases. When the liquid phase is denser than the solid phase, as in the case of gallium, the solid-liquid boundary slopes to the right with increasing pressure. This is because under high pressure, the substance prefers to be in the denser phase, which is the liquid phase for gallium.

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Key Concepts

Phase Diagrams

Density Anomalies

Melting Point and Phase Transition