chapter 12: liquids solids and phase changes
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36 Terms
similarities between liquids solids and gases
all consist of particles and are affected by temp and pressure; involve particles in motion
6 types of phase changes
melting, freezing, vaporization, condensation, sublimation, deposition
which phase changes are endothermic (absorb energy)
melting, vaporization, sublimation
which phase changes are exothermic (release energy)
freezing condensation and deposition
how do intermolecular forces affect phase changes
stronger IMFs require more energy to overcome leading to higher melting/boiling points
what happens in a closed container at liquid-vapor equilibrium
the rate of evaporation equals the rate of condensation the amount of liquid and vapor remain constant
vapor pressure
the pressure exerted by vapor in equilibrium with its liquid in a closed container
factors that affect vapor pressure
temp (increases vapor pressure) and strength of IMFs (IMF stronger= lower vapor pressure)
boiling point of a liquid
the temp at which its vapor pressure equals the external pressure
how do atmospheric pressure and IMFs affect boiling point
higher atmospheric pressure or stronger IMFs increase the boiling point
normal boiling point
the boiling point of a liquid at 1 atm pressure
two point clausius-clapeyron equation
ln(P2/P1)=ΔHvap/R(1/T1−1/T2)
what does the clausius calpeyron equation allow you to calculate
enthalpy of vaporization or vapor pressure at a given temperature
melting point of a substance
the temp at which solid and liquid are in equilibrium
how do IMFs influence melting point
stronger IMFs raise the melting point
what formula is used to calculate heat during a temp change
q=mcΔT
what formula is used to calculate heat during a phase change
q=nΔH
why does temp remain constant during a phase change
energy is used to break or form IMFs not increase kinetic energy
what is a phase diagram
graph that shows the physical state of a substance at various temps and pressures
where are solids located on a phase diagram
high pressure, low temp (upper left)
where are liquids located on a phase diagram
moderate pressure/ temp (center)
where are gases located on a phase diagram
low pressure, high temp (lower right)
triple point
the pressure and temperature where all three phases coexist
critical point
the temp and pressure beyond which a substance exists only as a supercritical fluid
what do phase boundaries on a diagram represent
conditions where two phases coexist in equilibrium
supercritical fluid
a state of matter that has properties of both liquids and gases and occurs above the critical point
melting
the phase change from solid to liquid when heat and energy breaks some intermolecular forces
vaporization
the phase change from liquid to gas; particles gain enough energy to escape into the vapor phase
sublimation
sloid turning directly to gas without becoming a liquid first
dynamic equilibrium in a closed system
when the rate of evaporation equals the rate of condensation; no net change in liquid or vapor
why does vapor pressure increase with temp
more particles have enough energy to escape the liquid increasing the amount of vapor
why is temp constant during a phase change
energy is used to break intermolecular forces, not raise temp
how do strong IMFs affect boiling and melting point
stronger IMFs= higher boiling/melting points because more energy is needed to break them
what does a phase diagram show
the phase of a substance at various temps and pressures
what is the critical point
the temp and pressure above which a substance becomes a super critical fluid
what is the triple point
the unique temp and pressure where sloid liquid and gas all exist at once in equilibirum