Based on the observations provided, we can create a heating curve for solid hydrogen:
Temperature (°C) | Time (minutes)
------------------------------------------
-263 | 0:00
-259 | 2:43 (melting point)
-253 | 10:36 (boiling point)
-245 | 18:00
The heating curve will have three distinct sections representing the three states of matter: solid, liquid, and gas. The time intervals can be determined based on the given data points.
On the curve, we would label:
1. Melting point (-259 °C): This is where hydrogen begins to change from a solid to a liquid state.
2. Boiling point (-253 °C): This is where hydrogen begins to change from a liquid to a gaseous state.
3. Solid phase: Labeled below the melting point.
4. Liquid phase: Between the melting and boiling points.
5. Gas phase: Above the boiling point.
Regarding the movement of energy during phase transitions, energy is either gained or lost during these transitions without affecting temperature. When transitioning from a solid to a liquid (melting), heat energy is absorbed by the substance without changing its temperature until all solid has converted into liquid form. Similarly, when transitioning from a liquid to a gas (boiling), heat energy is absorbed without causing an increase in temperature until all liquid has converted into gas form.
During these phase transitions, intermolecular bonds are broken or formed. In the case of hydrogen, as it melts, some of its intermolecular bonds break allowing molecules to move more freely while still being relatively close together in comparison to gases. As it boils and becomes a gas, most of its intermolecular bonds break, and the molecules move apart with increased kinetic energy.
I hope this explanation helps!