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Hemet High  Honors Chemistry
Name:________________________ Pd:___
Chapter 10 Homework Packet
All Notes Completed and Attached
Ch 10.1 pg 332 #2-6
Ch 10.2 pg 336 #4-6
Ch 10.3 pg 341 #2
Ch 10.4 pg 348 #5, 6
Ch 10.5 pg 351 #4, 6
and practice problems #1-2
Chapter 10 Review Worksheet
Due End of Class Today!
Final Packet
Test is on
Hemet High  Chemistry
10  States of Matter
Section 1: The Kinetic Molecular Theory of Matter
Based on the idea that particles of matter are always in _______________.
How it relates to gases:
____________________ = a hypothetical gas that perfectly fits all the assumptions of the KMT.
o No ideal gases actually exist; some come close though, which is why we learn this.
5 Assumptions
o Gases consist of large numbers of tiny particles that are far apart relative to their size.
o Collisions between gas particles and between particles and container walls are elastic collisions.
There is no net loss of total _____________________.
o Gas particles are in continuous, rapid, random _________. Thus, they possess kinetic energy.
o There are no forces of _________________ between gas particles.
o The ______________ of the gas depends on the average kinetic energy of the particles of the gas.
Properties of Gases:
No Definite ______________
Ability to be compressed _______________
No Definite ______________
Ability to _________ (fluid)
_________ Density
Real Gases
A gas that does not behave completely according to the assumptions of the __________________.
___________ gases and _____________ diatomic gases behave most like an ideal gas, as well as gases at
high ___________________ and low _____________________.
Section 2 and 3: Liquids and Solids
Properties of Liquids:
No Definite _____________
____________ Tension
___________ density
Mostly incompressible, so definite _______
Can Form ____________
Properties of Solids:
Definite _________
________ Density
Definite ___________
Defined _____________ Point
______ Rate of Diffusion
Type of Solids:
Crystalline Solids
o __________ Crystals
o __________ Crystals
o Covalent ____________ Crystals
o Covalent ___________ Crystals
Amorphous Solids
o Glass and ___________
Section 4: Changes of State
Matter on earth can exist in any state—gas, ______, or solid—and can change from one state to another.
The Possible changes of state are:
Change of State
Solid  Liquid
Solid  Gas
Liquid  Solid
Liquid  Gas
Gas  Solid
Gas  Liquid
Ice  Water
Dry Ice  CO2 Gas
Water  Ice
Water  Steam
Water Vapor  Ice
Water Vapor  Water
Endo or Exo?
Phase Diagram
A graph of _____________ versus ______________ that shows the conditions under which the phases of a
substance exist.
Tells you what __________ a substance will be in at a certain temperature and pressure.
______________________: the temperature and pressure conditions at which the solid, liquid, and vapor
phases of the substance can coexist at equilibrium.
______________________: the critical temperature and critical pressure of a substance.
______________________: the temperature above which the substance cannot exist as a liquid.
______________________: the lowest pressure at which the substance can exist as a liquid.
Phase Diagram of H2O
In which state is water at the following Temperatures and
Temperature Pressure
2.0 atm
0.5 atm
1.0 atm
Section 5: Changes of State
Structure of Water
Recall: Water has ____ Hydrogen and ____ Oxygen and has a ________ structure.
Ice forms a hexagonal pattern: Look at Fig 19 on pg 350
The empty spaces result in ice’s low density and are why it ___________.
Properties of Water
Pure water is transparent, _____________, tasteless and almost ___________________.
Water freezes and ice melts at 0°C and 1 atm.
Water boils at 100°C and 1 atm.
Molar enthalpy of fusion is 6.009 kJ/mol
Molar enthalpy of vaporization is 40.79 kJ/mol
Going from ice to water ___________ energy.
Going from water to steam __________ energy.
Going from water to ice ___________ energy.
Going from steam to water __________ energy.
The amount of energy is the ___________, it is just either required or released.
Calculating Amount of Energy
What quantity of energy is released when 804 g of water vapor condenses?
Calculating Mass from Energy
What mass of ice is required to release 2000 kJ of energy when melting?