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Summary General Chemistry A: Chemical Kinetics
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- Orange Coast College
Concise summary of Chemical Kinetics
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Reaction rate Differential rate law- is always positive - equation that relates rxn rate
- defined as: to concentration
,{A7=%[]_== la
- rate = k[A]n
-
. - zero order: rate of rxn is
independent of concentration
]
t§I=+µ- ¥ Rate-_k[A) 0--1<41--12
- in zero order, rate = constant
k
- disappearance rate refers - n = 0
to the neg. Equations (minus - first order: rxn rate
the coefficients) proportional to concentration of
-formation rate refers to reactant. When conc. Doubles,
the pos. Equations (minus rxn rate doubles. '
coefficients) - rate law: Rate -_k[ A]
[A] [ G] - n=1
t -second order: when conc.
y Doubles, rxn rate quadruples
-overall rxn is pos. -
-rate law: Rate __k[A]2
Quantity, but Reactant is - - n = 2
and [product] is + - for multiple reactants:
n
- average rxn rate: Rate -_K[ A]m[ B)
concentration change over
time within time interval
-instantaneous rxn rate:
concentration change at any
point in time. Determined from
slope of tangent
- if curve for conc. Vs. time
is for reactant:
Tangent slope =
-instantaneous rate = -slope
of tangent line
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