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Chem II Final Exam
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The energy of motion?
A. Kinetic
B. Potential
A. Kinetic
Stored energy?
A. Kinetic
B. Potential
B. Potential
Energy cannot be created or destroyed; it can only be converted from one form into another.
A. 3rd Law of Thermodynamics
B. 1st Law of Thermodynamics
C. 2nd Law of Thermodynamics
B. 1st Law of Thermodynamics
ΔE=E
_{final }
- E
_{initial }
A. Change in Time
B. Change in Rate
C. Change in Energy
C. Change in Energy
Energy leaving the system.
A. E
_{final}
> E
_{initial}
B. E
_{final}
< E
_{initial}
B. E
_{final}
< E
_{initial}
Energy entering the system.
A. E
_{final }
> E
_{initial}
B. E
_{final}
< E
_{initial}
A. E
_{final }
> E
_{initial}
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
F x d
Work
PV work formula.
w= -PΔV
Enthalpy equation.
ΔH=ΔE+PΔV
ΔH equals_____.
A. Products - Reactants
B. Reactants - Products
A. Products - Reactants
Internal energy formula.
ΔE=q-PΔV
Heat is represented by.
A. w
B. q
C. V
D. P
B. q
Energy is represented by.
A. q
B. w
C. V
D. E
D. E
The amount of heat required to raise the temperature of a certain object or amount by a certain temperature.
Heat capacity
Heat capacity is represented by.
A. V
B. C
C. q
D. P
B. C
Heat capacity formula.
C=q/ΔT
Specific heat formula.
q=C*m or mols*ΔT
The overall enthalpy change for a reaction is equal to the sum of the enthalpy changes for the individual steps.
Hess's law
For bond dissociation ΔH=______.
A. Products - Reactants
B. Reactants - Products
B. Reactants - Products
Spontaneous process happens when___
A. ΔH is - and ΔS is -
B. ΔH is - and ΔS is +
C. ΔH is + and ΔS is -
D. ΔH is + and ΔS is +
B. ΔH is - and ΔS is +
Nonspontaneous process happens when___
A. ΔH is - and ΔS is +
B. ΔH is + and ΔS is -
C. ΔH is - and ΔS is -
D. ΔH is + and ΔS is +
B. ΔH is + and ΔS is -
Free energy change formula.
ΔG=ΔH-TΔS
When ΔG is < 0 then the process is______.
A. nonspontaneous
B. at equilibrium
C. spontaneous
C. spontaneous
When ΔG is = 0 then the process is______.
A. nonspontaneous
B. at equilibrium
C. spontaneous
B. at equilibrium
When ΔG is > 0 then the process is______.
A. spontaneous
B. at equilibrium
C. nonspontaneous
C. nonspontaneous
When a process proceeds on its own without and external influence.
Spontaneous process
Entropy change for a reaction is ΔS=_________.
A. products - reactants
B. reactants - products
A. products - reactants
Entropy change formula for ideal gas.
ΔS°=nRln(Vfinal/Vinitial) or Pinitial/Pfinal
In any process, spontaneous or nonspontaneous, the total energy of a system and its surroundings is constant.
A. 1st Law of thermodynamics
B. 2nd Law of thermodynamics
C. 3rd Law of thermodynamics
A. 1st Law of thermodynamics
In an spontaneous process, the total entropy of a system and its surroundings always increases.
A. 3rd Law of thermodynamics
B. 2nd Law of thermodynamics
C. 1st Law of thermodynamics
B. 2nd Law of thermodynamics
The entropy of a perfectly ordered crystalline substance at 0 K is zero.
A. 1st Law of thermodynamics
B. 3rd Law of thermodynamics
C. 2nd Law of thermodynamics
B. 3rd Law of thermodynamics
Formula for entropy change in the surroundings for a reaction.
ΔS
_{surroundings}
=-ΔH/T
Formula for relationship between ΔG and K.
ΔG=-RTlnK
Formula for free energy change under nonstandard conditions.
ΔG=ΔG°+RTlnQ
Formula for standard free energy of a reaction.
ΔG°ΔG°products-ΔG°reactants
Rate Law.
Rate=Δ[A]/Δt or k[A]
^{m}
_{}
[B]
^{n}
Rate equals k
A. zeroth order
B. first order
C. second order
D. third order
A. zeroth order
Rate equals k[A]
A. second order
B. zeroth order
C. third order
D. first order
D. first order
Rate equals k[A][B]
A. first order
B. second order
C. zeroth order
D. third order
B. second order
Rate equals k[A][B]
^{2 }
A. third order
^{}
B. second order
C. first order
D. zeroth order
A. third order
Formula for half life of a first order reaction.
t
_{1/2}
=0.693/k
Equilibrium equation.
K
_{c}
=([C]
^{c}
[D]
^{d}
)/([A]
^{a}
[
^{}
B]
^{b}
Mole of solute divided by liters of solution.
Molarity
Equilibrium equation is______.
A. reactants over products
B. products over reactants
C. unknown
B. products over reactants
Gas constant R equals____.
A. 0.05672
B. 0.08503
C. 0.08206
C. 0.08206
A substance that can transfer H
^{+}
.
Bronsted-Lowry Acid
A substance that can accept H
^{+}
.
Bronsted-Lowry Base
H2O conjugate acid is?
H3O+
HA conjugate base is?
A-
NH3 conjugate acid is.
NH4+
H2O conjugate base is.
OH-
Chemical species who formulas differs only by one proton are called.
conjugate acid-base pairs
Author
bradolder
ID
346632
Card Set
Chem II Final Exam
Description
Gen Chem II final review cards.
Updated
2019-04-19T01:17:07Z
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