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Chemical Kinetics
- Gibb's Free Energy
- spontaneity of reaction:
Positive=not spontaneous
Negative=spotaneous
- + DG => endergonic-
consumes energy
-DG=> exergonic-
gives off energy
- + DG => endergonic-
consumes energy
-DG=> exergonic-
gives off energy
- spontaneity of reaction:
Positive=not spontaneous
Negative=spotaneous
- Collision Theory:
- rate of reaction is
proportional to the
number of collisions per
second btw the reacting
molecules. They must be
in the correct orientation
and energy.
- rate of reaction is
proportional to the
number of collisions per
second btw the reacting
molecules. They must be
in the correct orientation
and energy.
- Transition State Theory:
- when molecules collide with
energy higher than the
activation energy, they form
a transition state in which
old bonds are weakened by
new bonds forming.
- when molecules collide with
energy higher than the
activation energy, they form
a transition state in which
old bonds are weakened by
new bonds forming.
- Factors affecting reaction rate:
- *reaction
concentrations
*Temperature
*medium (polar
solvents etc.)
*catalysts
- *reaction
concentrations
*Temperature
*medium (polar
solvents etc.)
*catalysts
- Reaction Orders
- Zero Order:
- rate=k[A]^0 [B]^0=k
- rate=k[A]^0 [B]^0=k
- First Order:
- rate=k[A]^1
- rate=k[A]^1
- Second Order:
- rate=k[A]^1[B]^1 or
rate=k[A]^2
- rate=k[A]^1[B]^1 or
rate=k[A]^2
- Mixed Order: reactions
that change order over
time
- rate=k1[C][A]^2/k2=k3[A]
- rate=k1[C][A]^2/k2=k3[A]
- Zero Order:
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