Collision theory
Explore a bimolecular Arrhenius model and a separate illustration of collision energy and orientation.
About this tool
Choose an example or enter T, Eₐ and A, then calculate. The main value is the rate constant k. Calculation details contain exp(−q), q=Eₐ/(RT), RT and log₁₀k. Reset restores the standard example. Reload keeps validated inputs and view choices and requires Calculate again.
Arrhenius model
k=A exp(−Eₐ/(RT)), R=8.31446261815324J/(mol·K). Fixed bimolecular teaching reaction X+Y→products, with v=k[X][Y]. A and k use L mol⁻¹ s⁻¹. Concentrations are not supplied, so v is not calculated. No real reaction is claimed. T=100–3000K, Eₐ=0–300kJ/mol, A=10⁻¹²–10²⁰. A and Eₐ are constant over the temperature window. With Eₐ=0, k=A.
The graph shows log₁₀(k/[L mol⁻¹ s⁻¹]) against T from max(100,T/2) to min(3000,2T), with your temperature marked. It is a calculated curve, with no artificial minimum, measured data or inverse-temperature fit.
Collision illustration
E=0–600kJ/mol and orientation affect only the separate diagram. E<Eₐ means insufficient energy; E≥Eₐ with unfavorable orientation gives no bond; favorable orientation permits a bond. The checkbox does not change k: statistical orientation effects belong to A.
The slider or playback shows approach, then separation or joining. Three seconds are display time, not chemical time. Pause, tab switching and leaving the tool stop playback. There are no collision counters, molecular trajectories or predicted reaction probabilities. Even E=0 produces schematic motion.