Chemical Kinetics and Equilibrium Principles
Chapter 12: Chemical Kinetics
1. Reaction Rate & Stoichiometry
For aA+bB→cC+dD:
Rate = −(1/a)∗Δ[A]/Δt = −(1/b)∗Δ[B]/Δt = (1/c)∗Δ[C]/Δt = (1/d)∗Δ[D]/Δt
- Rate is always positive. Reactants are negative, products positive.
- Ex: 2NO2→2O2. If Rate of disappearance of NO2=0.010: Rate = −(1/2)∗(0.005 M/s. Rate of formation of O2=0.005. Rate of formation of NO=20.005 M/s=0.010.
2. Rate Laws & Reaction Order
Rate = k[A]m[B]n
- k: Rate constant (temp-dependent)
- m,n: Reaction orders (exp. Determined)
- Overall Order = m+n
- Method of Initial Rates: Compare two experiments where only one reactant's conc. Changes. (Rate/Rate) = ([A]2/[A]1)
- If Rate x2 when [A] x2 ⟹m=1 (1st order)
- If Rate x4 when [A] x2 ⟹m=2 (2nd order)
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