w = -PDV  or  -DngasRT
DSsurr = -DHsyst/T
qsurr = mCDt  or  CsetupDt
qsyst = -qsurr
DS°rxn = SS°products - SS°reactants
DH°rxn = SDH°fproducts - SDH°freactants
DG°rxn = SDG°fproducts - SDG°freactants
DSuniverse = DSsyst + DSsurr
DG°rxn = DH°rxn -TDS°rxn
DGrxn = DG°rxn +RT lnQ
DG°rxn = -RT lnKeq
ln(K2/K1) = (DH°/R) x (1/T1 - 1/T2)
 

A number of the questions on the exam were the same as those done in class.
(Use bond energies to find  DH° for H-H + H2C=CH2 --->  H3C-CH3)

Coffee Cup calorimeter question done in class.

similar K1 at T1 and K2 at T2.  Determine DG°, DH°, DS° etc.

1. Use Hess’s Law to find DH° for the reaction
   C2H2 (g) + 2H2 (g) <---> C2H6(g)

   from the following combustion data:

   C2H2 (g) + 5/2 O2 (g) <---> 2CO2 (g) + H2O (l)
   DH° = -1320 kJ

   H2 (g) + ½ O2 (g) <---> H2O (l)
   DH° = - 285 kJ

   C2H6(g) + 7/2 O2 (g) <---> 2CO2 (g) + 3H2O (l)
   DH° =- 1560 kJ

Answer: -330. kJ

   2.  When a 0.300 g sample of solid camphor (C10H16O) was burned in a bomb
   calorimeter, the temperature of the calorimeter and its contents increased by
   1.54 °C.  When an electric heater delivered 1500 W (1 W = 1 J/s)for 10 s to the
   calorimeter, its temperature changed from 25.30 °C to 27.30 °C.

   Calculate:
   a) the heat capacity of the calorimeter,
Answer: 7.50 kJ/oC
   b) the change in the internal energy, and
Answer: -11.55 kJ or -5861 kJ/mol
  c) the DH° of combustion per mole of camphor.
Answer: -5870 kJ/mol

   3.  For the reaction 2 SO2 (g) + O2 (g) <---> 2SO3 (g), Kc = 280 at 1000 K.
   a)  What is the value of DG° at 1000 K?
Answer: -10.2 kJ/mol
   b)  If 0.40 mol SO2, 0.18 mol O2, and 0.72 mol SO3 are mixed in a 2.50 L flask
        at 1000 K, in what direction will a net reaction occur?
Answer: Forward direction, DG = -15.2 kJ or Qc<Kc or Qp<Kp
                (note need to use Qp and Kp)

   4.  Calcium oxide (burnt lime) may be prepared by heating calcium carbonate
       (limestone) in a lime kiln, in the following reaction:

        CaCO3 (s) <---> CaO (s) + CO2 (g)

   The value of DH° for this reaction is +178.3 kJ; DS° is +0.1606 kJ/K.  Find the
   temperature at which this reaction becomes spontaneous if the partial pressure of CO2
   is 0.10 atm.
Answer: T = 992 K or 719 oC (0.10 atm is Kp at Temp T)
 


   7.  A 100.0 g sample of a substance with a density of 0.8200 g/cm³at 20.00 °C is
   heated to 150.00 °C under a constant pressure of 1 atm.  The sample absorbed 1.500 kJ
   of heat during this process and its volume increased by 10.00 %.  Find:
   a) q  Answer: 1.500 kJ
   b) w  Answer: -1.2 J
   c) DU, and Answer: 1.499 kJ
   d) DH. Answer: 1.500 kJ