Pt

Catalyst Reaction Kinetics & Activation Energy Simulator

Heterogeneous Surface Kinetics & Arrhenius Dynamic Lowering Model
Active Operating Point: Pt(111) Catalytic hydrogenation / CO oxidation preset
Catalytic Acceleration Factor: 1.42e+08×
Potential Energy Surface (PES)
Drag Node $E_a$
Reaction Coordinate → Potential Energy (kJ/mol) ↑ Uncatalyzed Ea: 120.0 kJ/mol Catalyzed Ea: 45.0 kJ/mol Reactants (A + B) Products (P)
💡 Direct Manipulation: Drag the neon cyan transition state node vertically to lower or raise activation energy barrier ($E_a$).
Matter.js 2D Micro-Particle Catalytic Chamber
Live Langmuir-Hinshelwood Engine
Gas Reactant A
Gas Reactant B
Adsorbed Intermediates
Desorbed Product P
Catalyst Bed Pt(111)
🔬 Gas phase collision dynamics, Langmuir adsorption onto active sites, catalytic intermediate bond formation, and thermal product desorption.
Kinetics Parameters & Catalyst Surface Poisoning
450 K
Thermal agitation & Boltzmann kinetic energy
2.5 atm
Gas particle density & surface flux
45.0 kJ/mol
Transition state stabilization energy
-35.0 kJ/mol
Active site chemisorption depth (Sabatier Principle)
Pt(111) Active Surface Sites Blockage / Poisoning Grid:
Site Coverage $\theta$: 0.00 | Poisoned: 0/20
Click individual active site blocks above to simulate local catalyst site poisoning (CO/Sulfur blockage).
Turnover Frequency (TOF) & Kinetics Telemetry
Catalyzed Rate ($k_{cat}$)
1.82e+07
$s^{-1} \cdot \text{site}^{-1}$
Uncatalyzed Rate ($k_{uncat}$)
0.128
$s^{-1}$ gas phase
Turnover Frequency (TOF)
14.8
reactions / site / sec
Conversion Yield
84.2%
Total Reactions: 0
Arrhenius Law Equation: $k = A \cdot e^{-\frac{E_a}{R \cdot T}}$
Lowering activation energy $E_a$ exponentially increases reaction rate constant $k$, enabling fast product formation at lower industrial temperatures.
Arrhenius Rate Plot ($\ln k$ vs $1/T$)
Slope = $-E_a / R$
Slope comparison: The lower slope of the catalyzed line (teal) illustrates the reduced activation energy barrier relative to uncatalyzed pathway (rose).
Catalysis Mechanics & Sabatier Principle Summary

Heterogeneous catalysts provide an alternative reaction pathway with a significantly lower activation energy ($E_a$). Reactants adsorb onto active metal surface sites (e.g. Pt(111)), undergo bond weakening, react via Langmuir-Hinshelwood kinetics to form transition state intermediates, and desorb as finished products. According to the Sabatier Principle, catalyst activity is optimized when binding energy ($E_{bind}$) is moderate—neither too weak to adsorb reactants nor too strong to desorb products.