Term
| How much heat is required to change 10 grams of water to steam at 100 ºC? |
|
Definition
| Heat of vaporization of water is 540 cal/g (10 g) (540 cal/g) = 5400 cal |
|
|
Term
| How much heat is required to melt 0.5 grams of ice at 0 ºC? |
|
Definition
| Heat of fusion of water is 80 cal/g (0.5)(80 cal/g) = 40 cal |
|
|
Term
| Define boiling point in terms of vapor pressure. |
|
Definition
| The temperature at which the vapor pressure over a liquid reaches atmospheric pressure. The substance boils (liquid to gas). |
|
|
Term
|
Definition
| The only temperature and pressure combination at which the three phases of a substance (solid, liquid, gas) can co-exist at equilibrium. |
|
|
Term
|
Definition
| Pressure the gas phase exerts on its liquid phase in a closed container. This pressure varies with temperature. |
|
|
Term
|
Definition
| The amount of energy required to change a gram of substance from solid to liquid at its melting point. |
|
|
Term
|
Definition
| The amount of energy required per gram to change a liquid to a gas at its boiling point. |
|
|
Term
|
Definition
|
|
Term
| Heat of Vaporization for water |
|
Definition
|
|
Term
|
Definition
| The temperature at which solid and liquid phases co-exist. |
|
|
Term
|
Definition
| The temperature above which the liquid phase of a substance can no longer exist. |
|
|
Term
|
Definition
| Minimum pressure required to liquify a gas at its critical temperature. |
|
|
Term
|
Definition
| When vapor pressure reaches atmospheric pressure, the temperature at which a liquid phase becomes a gas phase. assume pressure = 1 atm |
|
|
Term
|
Definition
| For a liquid in a closed container: when the rates of evaporation (liquid to gas) and condensation (gas to liquid) equalize, the concentration of each is stable. |
|
|
Term
|
Definition
| In a closed container where opposing changes are taking place at equal rates, the concentration of all components remains constant. |
|
|
Term
| Describe a phase change from liquid to gas. |
|
Definition
| When a molecule gains enough kinetic energy to overcome the intermolecular attractive forces within the liquid, it escapes the surface and becomes gas. |
|
|
Term
|
Definition
| A change from solid to vapor without the formation of liquid. Compounds which show sublimation: CO2, I2 |
|
|
