Heat is added to ice at 0 °C. Explain why the temperature of the ice does not change. What does change?
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Chemistry 2e · 10.3 Phase Transitions
Phase Transitions: practice problems
12 problems from the book, with its answers. Check your working, or have any of them explained to you on the whiteboard.
Exercises 33
Identify two common observations indicating some liquids have sufficient vapor pressures to noticeably evaporate?
Exercises 35
What is the relationship between the intermolecular forces in a liquid and its vapor pressure?
Exercises 37
Exercises 39
Exercises 41
Exercises 43
Exercises 45
Exercises 47
Exercises 49
Exercises 51
Exercises 53
Key terms · 13
- boiling point
- temperature at which the vapor pressure of a liquid equals the pressure of the gas above it
- Clausius-Clapeyron equation
- mathematical relationship between the temperature, vapor pressure, and enthalpy of vaporization for a substance
- condensation
- change from a gaseous to a liquid state
- deposition
- change from a gaseous state directly to a solid state
- dynamic equilibrium
- state of a system in which reciprocal processes are occurring at equal rates
- freezing
- change from a liquid state to a solid state
- freezing point
- temperature at which the solid and liquid phases of a substance are in equilibrium; see also melting point
- melting
- change from a solid state to a liquid state
- melting point
- temperature at which the solid and liquid phases of a substance are in equilibrium; see also freezing point
- normal boiling point
- temperature at which a liquid’s vapor pressure equals 1 atm (760 torr)
- sublimation
- change from solid state directly to gaseous state
- vapor pressure
- (also, equilibrium vapor pressure) pressure exerted by a vapor in equilibrium with a solid or a liquid at a given temperature
- vaporization
- change from liquid state to gaseous state
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