Chem II Final Exam

  1. The energy of motion?

    A.  Kinetic
    B.  Potential
    A.  Kinetic
  2. Stored energy?

    A.  Kinetic
    B.  Potential
    B.  Potential
  3. Energy cannot be created or destroyed; it can only be converted from one form into another.

    B.   1st Law of Thermodynamics
  4. ΔE=Efinal - Einitial

    A.  Change in Time
    B.  Change in Rate
    C.  Change in Energy
    C.  Change in Energy
  5. Energy leaving the system.

    A.  Efinal > Einitial
    B.  Efinal < Einitial
    B. Efinal < Einitial
  6. Energy entering the system.

    A.  Efinal > Einitial
    B.  Efinal < Einitial
    A.  Efinal > Einitial
  7. A function or property whose value depends only on the present state, or condition, of the system, not on the path used to arrive at that state.
    State function
  8. F x d
  9. PV work formula.
    w= -PΔV
  10. Enthalpy equation.
  11. ΔH equals_____.

    A.  Products - Reactants
    B.  Reactants - Products
    A.  Products - Reactants
  12. Internal energy formula.
  13. Heat is represented by.

    B.   q
  14. Energy is represented by.

    D.   E
  15. The amount of heat required to raise the temperature of a certain object or amount by a certain temperature.
    Heat capacity
  16. Heat capacity is represented by.

    B.   C
  17. Heat capacity formula.
  18. Specific heat formula.
    q=C*m or mols*ΔT
  19. The overall enthalpy change for a reaction is equal to the sum of the enthalpy changes for the individual steps.
    Hess's law
  20. For bond dissociation ΔH=______.

    A.  Products - Reactants
    B.  Reactants - Products
    B.  Reactants - Products
  21. Spontaneous process happens when___

    B.   ΔH is - and ΔS is +
  22. Nonspontaneous process happens when___

    B.   ΔH is + and ΔS is -
  23. Free energy change formula.
  24. When ΔG is < 0 then the process is______.

    C.   spontaneous
  25. When ΔG is = 0 then the process is______.

    B.   at equilibrium
  26. When ΔG is > 0 then the process is______.

    C.   nonspontaneous
  27. When a process proceeds on its own without and external influence.
    Spontaneous process
  28. Entropy change for a reaction is ΔS=_________.

    A.  products - reactants
    B.  reactants - products
    A.  products - reactants
  29. Entropy change formula for ideal gas.
    ΔS°=nRln(Vfinal/Vinitial) or Pinitial/Pfinal
  30. In any process, spontaneous or nonspontaneous, the total energy of a system and its surroundings is constant.

    A.   1st Law of thermodynamics
  31. In an spontaneous process, the total entropy of a system and its surroundings always increases.

    B.   2nd Law of thermodynamics
  32. The entropy of a perfectly ordered crystalline substance at 0 K is zero.

    B.   3rd Law of thermodynamics
  33. Formula for entropy change in the surroundings for a reaction.
  34. Formula for relationship between ΔG and K.
  35. Formula for free energy change under nonstandard conditions.
  36. Formula for standard free energy of a reaction.
  37. Rate Law.
    Rate=Δ[A]/Δt or k[A]m[B]n
  38. Rate equals k

    A.   zeroth order
  39. Rate equals k[A]

    D.   first order
  40. Rate equals k[A][B]

    B.   second order
  41. Rate equals k[A][B]2

    A.   third order
  42. Formula for half life of a first order reaction.
  43. Equilibrium equation.
  44. Mole of solute divided by liters of solution.
  45. Equilibrium equation is______.

    B.   products over reactants
  46. Gas constant R equals____.

    C.   0.08206
  47. A substance that can transfer H+.
    Bronsted-Lowry Acid
  48. A substance that can accept H+.
    Bronsted-Lowry Base
  49. H2O conjugate acid is?
  50. HA conjugate base is?
  51. NH3 conjugate acid is.
  52. H2O conjugate base is.
  53. Chemical species who formulas differs only by one proton are called.
    conjugate acid-base pairs
Card Set
Chem II Final Exam
Gen Chem II final review cards.