Integrated Rate Law for Zero-Order Reactions
[A] = -kt + [A]₀
Integrated Rate Law for First-Order Reactions
ln[A] = -kt + ln[A]₀
Integrated Rate Law for Second-Order Reactions
1/[A] = kt + 1/[A]₀
Unit of K for Zero-Order Reactions
molL⁻s⁻ or Ms⁻
Unit of K for First-Order Reactions
s⁻
Unit of K for Second-Order Reactions
mol⁻Ls⁻ or M⁻s⁻
Half-Life of Zero-Order Reactions
[A]₀/2k
Half-Life of First-Order Reactions
.693/k
Half-Life of Second-Order Reactions
1/k[A]₀
Relationship that Produces a Line for Zero-Order Reactions
[A] vs. t; slope = -k
Relationship that Produces a Line for First-Order Reactions
ln[A] vs. t; slope = -k
Relationship that Produces a Line for Second-Order Reactions
1/[A] vs. t; slope = k
What reacts faster, ionic or covalent molecules?
ionic
What reacts faster, simple or complex molecules?
simple
Factors that affect the Rate Constant
temperature and catalysts
Standard Arrhenius Equation
k = A e^(−Ea / RT)
Linear Arrhenius Equation
ln k = −(Ea / R)(1 / T) + ln A
Comparison Arrhenius Equation
ln(k2 / k1) = −(Ea / R)(1 / T2 − 1 / T1)
