13. Liquids, Solids & Intermolecular Forces

Calculate the amount of heat (in J) required to heat 2.00 grams of ice from −12.0℃ to 88.0℃.
The heat of fusion of water is 6.02 kJ/mol, the specific heat capacity of ice is 2.09 J/g ▪℃ and the specific heat capacity of water is 4.184 J/g ▪℃.

In a phase diagram, at what temperature does the solid phase begin to melt?

Which of the following correctly describes a key difference between the phase diagrams of water and carbon dioxide?

In a typical phase diagram of water, which numbered point on the graph represents the phase change known as melting?

In a phase diagram for CO_2, which point represents the critical point?

Which of the following changes occurs as a solid is heated?

Which of the following factors can cause a substance to transition between the solid and liquid states?

When water vapor is cooled at constant pressure, which phase change is most likely to occur?

Which statement best describes the difference between sublimation and deposition in a phase diagram?

Which of the following best describes the process of melting in a phase diagram?

For a given substance:

Which of the following is the best example of water changing from a liquid to a gas?

Which best describes the behavior of atoms in a solid substance that is melting into a liquid?

In a typical phase diagram, in which region does a substance exist in both the solid phase and the liquid phase simultaneously?