CHM2CH19

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Author:
pamichael5350
ID:
118193
Filename:
CHM2CH19
Updated:
2011-12-10 23:49:00
Tags:
chemistry thermodynamics
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Description:
Chemical Thermodynamics
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  1. Define enthalpy:
    EQUATION
    • Measure of heat gained or lost.
    • H=E+PV
  2. What change in enthalpy makes reaction endothermic vs exothermic?
    • change in H = positive = endothermic
    • change in H = negative = exothermic
  3. Equation to find change in enthalpy
    change in H = H products - H reactants
  4. Define entropy:
    EQUATION
    • measure of the randomness or disorder of a system
    • S = Sum n S products - Sum m S reactants
  5. Equation to find change in entropy
    change in S = S final - S initial
  6. What causes increases in entropy?
    (increases randomness)
    • - increase in temperature
    • - increase in volume
    • - increase in # of molecules or gas moles
    • - gases formed from liquids or solids
    • - liquids or solutions formed from solids
    • - solid disolved in solid
  7. Gibbs Free Energy Equation
    change G = change H - T (change S)

    change G = Sum n G products - Sum m G reactants
  8. What value of G makes reaction spontaneous?
    • change G = negative = spontaneous
    • change G = positve = non spontaneuos
    • change G = zero = equilibrium
  9. Effects of H and S on g
    • H = neg S = pos G = neg
    • spontaneous at any temp

    • H = pos S = neg G= pos
    • non-spontaneous at any temp

    • H = neg S= neg : depends on TEMP
    • Temp is high: G = pos
    • Temp is low: G = neg
  10. Free energy equations using K
    G = -RT ln K

    G = G standard + RT ln Q
  11. First Law of Thermodynamics
    • Energy cannot be created or destroyed.
    • The total energy of the universe is constant.
  12. Second Law of Thermodynamics
    The entropy of the universe increases for spontaneous processes and the entropy of the universe does not change for reversible processes.
  13. Third Law of Thermodynamics
    The entropy of a pure crystalline substance at absolute zero is zero.

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