Chemical Reaction Rate Calculator
First Order Kinetics
ln[A] = ln[A]₀ - kt
Second Order Kinetics
1/[A] = 1/[A]₀ + kt
Zero Order Kinetics
[A] = [A]₀ - kt
Arrhenius Equation
k = A·exp(-Ea/RT) — Temperature dependence of rate
Formula
Zero: [A] = [A]₀ - kt | First: [A] = [A]₀·e^(-kt) | Second: 1/[A] = 1/[A]₀ + kt | Arrhenius: k = A·e^(-Ea/RT)
Frequently Asked Questions
What is a reaction rate?
Reaction rate is the change in concentration per unit time. Rate = -Δ[reactant]/Δt = +Δ[product]/Δt. The rate law: Rate = k[A]^n, where k is the rate constant and n is the reaction order.
How do reaction orders differ?
Zero order: rate is constant, [A] decreases linearly, t½ = [A]₀/2k. First order: rate depends on [A], exponential decay, t½ = ln(2)/k. Second order: rate depends on [A]², t½ = 1/(k[A]₀).
What is the Arrhenius equation?
k = A·e^(-Ea/RT) relates the rate constant to temperature. Ea is activation energy, A is the pre-exponential factor. Higher Ea = more temperature-sensitive. A 10°C increase typically doubles to triples the rate.
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