Phases

Phases

Phases

• Phase- and part of a system that has uniform composition and properties

• COndensation- process by which a gas changes to a liquid

• vaporization - process by which a liquid changes to a gas

• Equilibrium- condition where two opposing changes happen at the same rate. liquid to gas and gas to liquid

• Equilibrium vapor pressure- pressure exerted by the vapor in equilibrium with its liquid at a given temperature

• Volatile liquids- liquids that evaporate readily, have weak attractive forces between particles

Phases

• Boiling- conversion of liquid to vapor within the liquid as well as its surface

• Boiling point- equilibrium vapor pressure equals atmospheric pressure

• molar enthalpy of vaporization- amount of energy needed to vaporize one mole of a liquid at the liquids boiling point at constant pressure

Open Ended

Describe the difference between evaporation and boiling(there is a difference)

Phases

• freezing point- temp at which solid and liquid are in equilibrium at 1 atm

• molar enthalpy of fusion- amount of energy as heat required to melt one mole of solid at the solids melting point

• sublimation- solid to gas

• deposition- gas to solid

Multiple Choice

Molar enthalpy of fusion for ice is 6.01 kj/mol. How much energy is required for .5 mol of ice to melt?

• 6.01 kj

• 3 kj

• .5 kj