1. Define Thermochemistry:
    –The study of the heat flow that accompanies chemical reactions.
  2. Define Energy and heat in thermochemistry
    Energy–The capacity to do work

    Heat–A particular form of energy that is transferred from a body at a high temperature to one at a lower temperature when they are brought into contact with each other
  3. Define Kinetic energy
    Kinetic energy is energy of motion or energy that is being transferred.
  4. Define Thermal energy.
    Thermal energy is the energy associated with temperature. Thermal energy is a form of kinetic energy
  5. What is ΔX?
    X Final - X inital
  6. Is heat flow a state property?
    –Heat flow is NOT a state property!! It depends on how the process is carried out
  7. Heat is given the symbol q.
    When is  q negative or positive?
    • –q is positive when heat flows into the system from the surroundings
    • –q is negative when heat flows from the system into the surroundings
  8. Changes of state Diagram
    Image Upload 1
  9. 1 cal = _ Joules
    1 kcal = _ kJ
    1 food Calorie = _ Kcal
    • 4.184
    • 4.184
    • 1
  10. Expand the define these 2 formulas.

    q = CΔt
    q = mcΔt
    C=heat capacity

    • Q = mc∆TQ = heat energy (Joules, J)
    • m = mass of a substance (kg)
    • c = specific heat (units J/kg∙K)
    • ∆ is a symbol meaning "the change in"∆T = change in temperature (Kelvins, K)
  11. The formula for kinetic energy is:
    KE=  (1/2)m⋅v^2

    • m = kg
    • v = m/s
  12. 1 mile is how many km?
  13. 1 pound is how many grams?
    454 grams
  14. w=Fd

    Expand these formulas for work.
    • m = mass in kg
    • g = gravity = 9.81 m * s ^-1
    • F = force in Newtons
    • w = work in joules
  15. The formula for velocity.
    v = sqaure root(2E/m)

    m = meters
  16. The ideal gas Law
    PV = nRT

    • P = Atm
    • V= Liters
    • n = moles
    • R = 0.08206 for atm 8.314 for joules
    • T = temperature in Kelvins
  17. kJ to Liter * atm
    (0.101 kJ=1 L⋅atm)
  18. w=−PΔV

    • p= liters * atm
    • v - change in volume (Liters)
  19. Fahrenheit to Celsius
    (1.8)C + 32 = F
  20. What is the specific heat of water?
    4.184 j/g ºCelsius
  21. Grams to moles
    Moles x Molecular weight = Grams
  22. Calorimeter to q formula.
    q reaction =  -c (specific heat) calorimeter Δt

    qreaction = -m water X 4.18 J/(g . °C) x Δt
  23. Formulas for enthalpy.
    Heat Flow.
    • –Enthalpy is a state variable
    • –ΔH = Hproducts – Hreactants

    qreaction = ΔH = H products – H reactants
  24. Rules of Thermochemistry
    1. The magnitude of ΔH is directly proportional to the amount of reactant or product

    2. ΔH for the reaction is equal in magnitude but opposite in sign for ΔH for the reverse of the reaction

    3.The value of ΔH is the same whether the reaction occurs in one step or as a series of steps This rule is a direct consequence of the fact that ΔH is a state variableThis rule is a statement of Hess’s Law
  25. The formula for enthalpies of formation.
    • –Enthalpies of Formation can be used to calculate ΔHfº for a reaction.
    • –To do this, apply this general rule:
    • –The standard enthalpy change, ΔHº, for a given thermochemical equation is equal to the sum of the standard enthalpies of formation of the product compounds minus the sum of the standard enthalpies of formation of the reactant compounds

    ΔHº = ∑ΔHfº products - ∑ ΔHfº reactants

    Note—elements can be omitted because ΔHfº = 0 for elementsΔH°f H+ (aq) = 0
  26. Relationship between ΔH and ΔE
    H = E + PV

    ΔH = ΔE + Δ(PV)

    • Remember the Idea gas law
    • The PV product is important only where gases are involved; it is negligible when only liquids or solids are involved
    • Δ(PV) = ΔngRT
    • –Δng is the change in the number of moles of gas when the reaction takes place

    ΔH = ΔE + ΔngRT
  27. ΔE=q + w
    • E = Joules
    • q = heat
    • w = work
  28. x kJ=1 L⋅atm
    0.101 kJ=1 L⋅atm
Card Set
Chapter 6