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WorksheetsChanges of State
Total questions: 20
Worksheet time: 15mins
Define: volatile liquids
A liquid that evaporates readily or at low temperature.
One in which there is no net loss of total kinetic energy.
A substance that can flow and therefore take the shape of its container.
The amount of energy as heat required to evaporate 1 mol of a liquid at a constant pressure and temperature.
Define: equilibrium vapor pressure
A liquid that evaporates readily or at low temperature.
The vapor pressure of a system at equilibrium.
The change of state from gas to liquid.
The amount of energy as heat required to evaporate 1 mol of a liquid at a constant pressure and temperature.
Define: condensation.
The process by which a liquid or solid changes to a gas.
The process by which particles escape from the surface of a nonboiling liquid and enter the gas state.
The physical change of a liquid to a solid by removal of energy as heat.
The change of state from gas to liquid.
Define: nonvolatile liquid
Substances that retain certain liquid properties even at temperatures at which they appear to be solid.
Ones in which the particles are arranged randomly.
A vapor that doesn’t evaporate rapidly or at a low temperature.
A substance in which the particles are arranged in an orderly, geometric, repeating pattern.
Define: molar enthalpy of vaporization
The amount of energy as heat required to evaporate 1 mol of a liquid at a constant pressure and temperature.
A dynamic condition in which two opposing changes occur at equal rates in a closed system.
The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature.
The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature.
What doesn't occur at higher elevations?
Atmospheric pressures are lower.
Nothing.
Foods take longer to cook.
Liquid boil at a lower temperature.
What isn't a part of liquid-vapor equilibrium?
Evaporation and condensation rates are equal.
The concentrations of reactants and products change.
Must occur in a closed system.
Substances change back and forth between states at equal speeds.
What doesn't occur during freezing?
Molecules slow down.
Substance gets slippery and wet.
Molecules come to fixed positions.
There's a loss of energy.
Melting and freezing...
are the same thing.
must occur in a closed system.
occur at a constant temperature.
don't continuously absorb/lose heat.
When gas changes straight into a solid is known as...
sublimation.
condensation.
deposition.
evaporation.
What is the point where a substance exists in all three phases at once?
Triple Point
Pressure Point
Critical Point
Temperature Point
_____ diagrams show the relationships between states as a function of pressure and temperature.
Equilibrium
State
Concept
Phase
What is a unique property of CO2 in regards to phases. (Think of the phase diagram of CO2.)
It never goes into a solid phase.
It never goes into a liquid phase.
It never goes into a gas phase.
Nothing.
Which best fits a solid?
Far apart particles.
Loose particles.
Tightly packed particles.
None.
Which best fits a liquid?
Far apart particles.
Loose particles.
Tightly packed particles.
None.
Which best fits a gas?
Far apart particles.
Loose particles.
Tightly packed particles.
None.
Define: molar enthalpy of fusion.
The vapor pressure of a system at equilibrium.
A liquid that evaporates readily or at low temperature.
The change of state from gas to liquid.
The amount of energy needed to change one mole of a substance from the solid phase to the liquid phase at constant temperature and pressure.
Can boiling water and steam coexist?
Yes.
No.
How do you convert to find the energy required to vaporize a given amount of a substance?
g > kJ
g > mol > kJ
kJ > mol > g
g > mol
When solid changes straight into a gas is known as...
sublimation.
condensation.
deposition.
evaporation.
