CHEM1102 Kinetics Equations
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Rate =
-Δ[reactant]
=
+Δ[product]
aΔt bΔt
= k[A]
^{m}
x [B]
^{n}
First Order Reactions
ln([A]
_{t}
) =
ln([A]
_{0}
) - kt
First Order Reactions
t
_{1/2}
=
0.693/k
First Order Reactions
Remaining Fraction?
ln (1/(remaining fraction)) = kt
Second Order Reactions
rate =
k[A]
^{2}
Second Order Reactions
1/[A]
_{t}
=
1/([A]
_{0}
) + kt
Activation Energy
ΔE =
E
_{prod}
- E
_{reactants}
= ΔH
Arrhenius Equation
f =
e
^{(-Ea)/(RT)}
Arrhenius Equation
lnK =
lnA - Ea/RT
Card Set Information
Author:
Boost
ID:
247891
Filename:
CHEM1102 Kinetics Equations
Updated:
2013-11-19 23:16:54
Tags:
chemistry 1b equations Kinetics
Folders:
Description:
Kinetics equations
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