Unit 6 Review
Chemistry II
****Bring a scientific calculator
Definitions
 Energy
 Temperature
 Heat
 Exothermic
 Endothermic
 Enthalpy
 Entropy
 Specific heat
 Heat of Formation
 Heat of Combustion
 Heat of Fusion
 Heat of Vaporization
 Thermodynamics
 Joule
 Calorimeter
Be able to:
 Calculate Hess’ Law
 Calculate ∆H given values from table
 1st law of thermodynamics
 2nd law of thermodynamics
 Calculate n, q, m, C, ∆T given various values
 When a spontaneous rxn occurs (decrease in energy, increase in disorder)
 Example of increasing entropy (dissolving crystals)
 Exothermic and Endothermic Reactions
o Values of H
o Where the energy term goes in a thermochemical equation
o Energy profile diagram
 Factors that affect spontaneity
 Calculate the energy of a phase change
 Calculate molar heat of fusion and vaporization
 Calculate molar mass given the molar heat of fusion or heat of fusion
 Calculate ∆G and determine if a rxn is spontaneous
 Be able to draw a phase change diagram
Formulas and Data given on test:
q
Cp = -------m x ΔT
q = mC∆T
Cp = specific heat (J/g · K)
q = heat lost or gained (J)
m = mass of sample (g)
ΔT = change in temperature (K)  Tf - Ti
q
Cp = -------n x ΔT
q = nC∆T
Cp = specific heat (J/mol · K)
q = heat lost or gained (J)
n = number of moles (mol)
ΔT = change in temperature (K)  Tf - Ti
ΔH = Hproducts - Hreactants
Specific Heat of water
3.77 x 10-2 KJ/mol ▪ ̊C
or 2.09 J/g ▪ ̊C
Liquid = 7.54 x 10-2 KJ/mol ▪ ̊C
or 4.18 J/g ▪ ̊C
3.63 x 10-2 KJ/mol ▪ ̊C
or 2.01 J/g ▪ ̊C
Solid =
Gas =
Water = Hv (heat of vaporization) = 40.7 KJ/mol
Water = Hf (heat of fusion) = 6.01 KJ/mol
∆G = ∆H - T∆S