Chemical Kinetics Calculators

Chemical kinetics calculators provide essential computational tools for reaction rates, rate constants, half-lives, and activation energy determinations. These specialized calculators help students and researchers analyze reaction mechanisms, predict concentration changes over time, and understand temperature effects on reaction rates with precision and accuracy.

Use comprehensive kinetics tools for Arrhenius equation calculations, reaction order determinations, integrated rate law applications, and catalyst effect estimations. Each calculator implements fundamental kinetic principles including collision theory, transition state theory, and rate laws to support accurate laboratory work and kinetic analysis in chemical systems.

⚠ Disclaimer: This calculator provides results based on standard formulas and simplified assumptions. It is intended for educational purposes only and should not be used for professional, medical, industrial, or experimental applications without expert verification.

Rate Constant from Concentration/Time

Initial concentration [A]₀ (M) Final concentration [A] (M) Time (s)

For first order: k = (1/t) ln([A]₀/[A])

Half-life Calculator (First-order)

Rate constant k (s⁻¹)

t₁/₂ = 0.693 / k

Half-life Calculator (Second-order)

Rate constant k (M⁻¹·s⁻¹) Initial concentration [A]₀ (M)

t₁/₂ = 1 / (k [A]₀)

Reaction Order Estimator (from Data)

Rate₁ (M/s) Rate₂ (M/s) [A]₁ (M) [A]₂ (M)

n = log(rate₂/rate₁)/log([A]₂/[A]₁)

Integrated Rate Law Calculator

Order (1 or 2) Initial concentration [A]₀ (M) Time t (s) Rate constant k

1st: [A]=[A]₀ e⁻ᵏᵗ; 2nd: 1/[A]=1/[A]₀ + kt

Arrhenius Equation Calculator

Frequency factor A Activation energy Ea (kJ/mol) Temperature (K)

k = A·exp(-Ea/RT)

Activation Energy Estimation

k₁ k₂ T₁ (K) T₂ (K)

Ea = R ln(k₂/k₁) / (1/T₁ – 1/T₂)

Temperature Effect on Rate

k₁ T₁ (K) T₂ (K) Activation energy Ea (kJ/mol)

k₂ = k₁·exp[Ea/R(1/T₁ – 1/T₂)]

Rate → Concentration Change Calculator

Rate v (M/s) Time Δt (s)

Δ[A] = rate × Δt

Pseudo-first-order Approximation

Rate constant k (s⁻¹) Time t (s) Initial concentration [A]₀ (M)

[A] = [A]₀ e⁻ᵏᵗ

Initial Rate Method Calculator

Rate₁ (M/s) Rate₂ (M/s) [A]₁ (M) [A]₂ (M)

Order = log(r₂/r₁) / log([A]₂/[A]₁)

Rate Constant Units Converter

Order (n)

Units depend on order: M^(1-n)·s⁻¹

Reaction Time to Completion

Initial concentration [A]₀ (M) Final concentration [A] (M) Rate constant k (s⁻¹)

First-order: t = ln([A]₀/[A]) / k

Zero-order Reaction Calculator

Initial [A]₀ (M) Rate constant k (M/s) Time t (s)

[A] = [A]₀ – kt

First-order Reaction Calculator

Initial [A]₀ (M) Rate constant k (s⁻¹) Time t (s)

[A] = [A]₀ e⁻ᵏᵗ

Second-order Reaction Calculator

Initial [A]₀ (M) Rate constant k (M⁻¹·s⁻¹) Time t (s)

1/[A] = 1/[A]₀ + kt

Catalyst Effect on Rate Calculator

Rate constant without catalyst k₁ Rate constant with catalyst k₂

Rate enhancement = k₂/k₁

Collision Frequency Approximation

Concentration [A] (M) Concentration [B] (M) Rate constant k (M⁻¹·s⁻¹)

Rate ≈ k[A][B]

Molecularity Estimation

Number of reactant molecules colliding

Molecularity = number of species in elementary step

Half-life to Rate Constant Conversion

Half-life t₁/₂ (s)

For first-order: k = 0.693 / t₁/₂