Heat is applied to an ice cube in a closed container until only steam is present. Draw a representation of this process. What happens to the size of the molecules and total mass of the sample?

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In this process, the heat is applied to an ice cube in a closed container, causing the ice to undergo a phase change from solid to liquid and finally to gas. Here's a representation of this process:

[Ice Cube] --> [Water] --> [Steam]

Now, let's discuss what happens to the size of the molecules and the total mass of the sample during this transformation.

1. Size of Molecules:
As heat is applied to the ice cube, the kinetic energy of the molecules increases. This causes the molecules to vibrate more vigorously, breaking the intermolecular forces that hold the solid ice together. As a result, the molecules become less tightly packed and gain more freedom of movement, enabling them to slide past each other.

When the ice melts and turns into liquid water, the size of the molecules remains relatively unchanged. The water molecules are still closely packed but have more free motion compared to the solid state.

When further heat is applied, the liquid water molecules gain even more energy and move even more rapidly. The increased energy allows the water molecules to overcome intermolecular forces and escape the liquid phase, forming water vapor or steam. In the gaseous state, the water molecules are more spread out and have higher kinetic energies, moving independently and chaotically.

To summarize, as the ice cube transitions from solid to liquid and then to gas, the size of the water molecules remains relatively constant, but their arrangement and freedom of movement change.

2. Total Mass:
During the phase change, the total mass of the sample remains constant. This principle is known as the law of conservation of mass, which states that mass cannot be created or destroyed in a closed system. So, regardless of whether the water is in the solid, liquid, or gaseous state, the total mass of the sample, including the molecules, remains the same throughout the entire process.

In conclusion, as heat is applied to an ice cube, it undergoes a phase change, resulting in the molecules transitioning from a solid to a liquid state and then to a gaseous state. The size of the molecules remains relatively constant, while their arrangement and freedom of movement change. Meanwhile, the total mass of the sample remains constant due to the law of conservation of mass.