Ch. 12 Liquids and Solids,
Liquids
Fluid: ______________________________________
High Density _______________________________
Relative Incompressibility ___________________________________
Ability to diffuse _______________________________
Surface Tension ___________________________________
Capilary Action ___________________________________
Evaporation ___________________________________
Boiling ___________________________________
Solids pp 370
Crystals
Ionic ___________________________________
Covalent Network ___________________________________
Metallic ___________________________________
Covalent ___________________________________
Change of State
Equilibrium ___________________________________
Equilibrium vapor Pressure of a Liquid (Fig. 12-12 p. 377)
Volatile liquids ___________________________________
Boiling and C _______________ occur when ____________________
Molar Heat of Vaporization (Hv =40.7 kJ/mol)
Freezing and Melting ___________________________________
Molar Heat of Fusion (Hf =334 J/g)
Add Heat from the system: 

Remove Heat from the system: 

Freezing is an process
Melting is an process
Q = m Cp T
M = ______________Cp = ______________ T _______________
Use absolute value for T
Use correct sign of Q by Exo/Endo determination:
q = ΔH (mass/molar mass) for evaporation or fusion
http://www.chemteam.info/Thermochem/Time-Temperature-Graph.html
Be careful using g or mol
q = ΔHvap (mass/molar mass) = 40.7 kJ / mol evaporation or condensation
Example #1 49.5 g of H2O is being completely boiled at its boiling point of 100 °C. How many kJ is
required? Ans. 111.9 kJ
Example #2: 80.1 g of H2O exists as a gas at 100 °C. How many kJ must be removed to turn the
water into liquid at 100 °C.
Solution: note that the water is being condensed. The molar heat of vaporization value is used at the
solid-liquid phase change, REGARDLESS of the direction (boiling or condensing).
Example #3: calculate the heat of vaporization for water in J/g
Ans. 2260J/g
q = ΔHfus (mass/molar mass) = 6.02 kJ/mol fusion solidification or melting
Example #1: 31.5 g of H2O is being melted at its melting point of 0 °C. How many kJ is required?
Ans. 10.5 kJ
Example #2: 53.1 g of H2O exists as a liquid at 0 °C. How many kJ must be removed to turn the
water into a solid at 0 °C
Solution: note that the water is being frozen and that there is NO temperature change. The molar
heat of fusion value is used at the solid-liquid phase change, REGARDLESS of the direction (melting
or freezing).
Example #3: calculate the heat of fusion for water in J/g
Ans. 334J/g
Other sections of graphs have different Cp values
Cp for solid water = 2.06 J/ g °C
Cp for liquid water = Cp = 4.184 J/ g °C
Cp for solid water = 1.87J/ g °C
Problem #1: Calculate the heat necessary to raise 27.0 g of water from 10.0 °C to 90.0 °C
The important factor about this problem is that ONLY temperature change is involved. Therefore, the
equation to use is: q = (mass) (Δt) (Cp)
Four Equations Needed Problem #1: 33.3 grams of ice at 0.00 °C has heat added to it until steam
at 150.0 °C results. Calculate the total energy expended. (Hint: melt, raise, boil, raise.)
and Ch.17 Thermochemistry
Define the following terms:
Thermochemistry ______________________________
Heat _____________________________
Temperature _______________________
Calorimeter _________________________
Specific heat_____________________________
Specific heat of Al ____________________________
As the temperature of 50.0 grams of Al changes from 20.0 C to 70.0 C, how much energy is required?
___________________
Specific heat of Pb ___________________
As the temperature of 50.0 grams of Pb changes from 20.0 C to 70.0 C, how much energy is required?
___________________
How much heat can be gained by Pb when Pb changes Temperature from 300 K to 350 K
Write the thermochemical reaction for the synthesis of water (p.515) ___________________
What is a thermochemical equation? _________________________
What is enthalpy? ____________________________
Draw the exothermic reaction pathway – label everything from Fig. 17-2
Draw the endothermic reaction pathway – label everything from Fig. 17-3
What is the molar heat of formation? ________________________________________
Skip the rest of this unit 17-1
Section 17-2 Driving Force of Reactions
What is the relationship between enthalpy and reaction tendency?
_________________________________________________________________________________
What is the relationship between entropy and reaction tendency?
_________________________________________________________________________________
What is entropy? ____________________________________________________
What is free energy? ____________________________
Write the reaction for free energy ________________________________________
If free energy has a positive value, is the reaction spontaneous?
If free energy has a negative value, is the reaction spontaneous?
If a reaction occurs at 25 C, and releases 160 kJ/mol of energy and has an entropy value of positive 50
J/mol K, what is the free energy of the reaction? Is it spontaneous?
Section 17-3 Reaction Process
What is a reaction mechanism? ____________________________________________________
What is collision theory? ___________________________________________
What is activation energy? _____________________________________________
Draw Figure 17-10, label all parts well, p. 534
Do sample problem 17-5 p.536, label well, then do the practice problem on p. 537
Section 17-4 Reaction Rate
Define reaction rate _________________________________________________
Define chemical kinetics ________________________________
Rate Influencing factors
List:
Draw Figure 17-15 with reaction with no catalyst and the reaction with one catalyst, label all parts well.
Skip Rate Laws