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CHEMISTRY • KINETICS
Reaction Rate
Separate temperature, activation energy, concentration and reaction order. Compare two temperatures on the same Arrhenius response and solve for a requested relative rate.
● LIVE KINETICS STATEreaction rate
Thermal populationReference temperatureActivation barrier
Rate index—
Relative k—
Reference rate—
Target error—
Reaction order—
Ea/RT—
Keep the two effects distinct
Temperature changes the Arrhenius rate constant while concentration is applied through the selected reaction order. The plotted quantity is a relative rate index anchored to the same Arrhenius model at 298.15 K.
Fast investigations
- Raise temperature while keeping Ea and concentration fixed.
- Raise Ea while keeping temperature fixed.
- Double concentration for zero-, first- and second-order cases.
- Find two different parameter combinations that reach the same target rate.
LEARN WITH THE SIMULATION
Understand Reaction Rate by experimenting.
START HERE
Reaction rate depends on both molecular encounters and the fraction of collisions energetic enough to cross an activation barrier. The Arrhenius equation captures the strong temperature dependence of many rate constants.
BUILD THE IDEA
What you should understand first
- See how activation energy affects the rate constant.
- Compare temperature effects through the Arrhenius exponential.
- Connect reaction order to concentration dependence.
TRY IT YOURSELF
Why can a modest temperature increase strongly accelerate a reaction?
- Record the rate at a chosen temperature.
- Increase temperature while holding activation energy and concentration fixed.
- Compare the rate ratio, then repeat with a larger activation energy.
Read the visual:
The Arrhenius exponential makes the fraction of sufficiently energetic events rise rapidly with temperature, especially for larger activation barriers.
WHY IT WORKS 01
See how activation energy affects the rate constant.
Reaction rate depends on both molecular encounters and the fraction of collisions energetic enough to cross an activation barrier. The Arrhenius equation captures the strong temperature dependence of many rate constants. Focus on the relationship between the controlled variable and the measured response rather than treating the visual change as the explanation.
WHY IT WORKS 02
Compare temperature effects through the Arrhenius exponential.
The Arrhenius exponential makes the fraction of sufficiently energetic events rise rapidly with temperature, especially for larger activation barriers. Use an extreme or boundary setting after the baseline trial to check whether the same reasoning still holds.
DO NOT MIX THESE UP
Common misconception
Reaction order is an empirical kinetic property, not always the same as a balanced-equation coefficient. Catalysts change pathways and activation barriers rather than equilibrium constants. This model uses a simplified pre-exponential factor.
PRACTICE CHALLENGE
Why can a modest temperature increase strongly accelerate a reaction?
- Record the rate at a chosen temperature.
- Increase temperature while holding activation energy and concentration fixed.
- Compare the rate ratio, then repeat with a larger activation energy.
Reveal the reasoning
The Arrhenius exponential makes the fraction of sufficiently energetic events rise rapidly with temperature, especially for larger activation barriers. Reaction order is an empirical kinetic property, not always the same as a balanced-equation coefficient. Catalysts change pathways and activation barriers rather than equilibrium constants. This model uses a simplified pre-exponential factor.
MODEL BOUNDARIES
What this simulation assumes
Every simulation simplifies reality or a mathematical system. These are the assumptions and limits to keep in mind while interpreting the results.
Model assumptions
- Temperature dependence follows a simplified Arrhenius relationship.
- Rate depends on a single concentration raised to an integer reaction order of 0, 1 or 2.
- Activation energy and reaction order are treated as constant over the experiment.
Model limitations
- Real mechanisms can involve multiple elementary steps, catalysts and several reactants.
- The model reports a relative rate scale and does not derive a complete kinetic mechanism from molecular collisions.
CONNECT IT
Where this matters
- Chemical reactors
- Food and material degradation
- Catalysis
WORDS THAT MATTER
Key vocabulary
- Activation energy
- Energy barrier associated with a reaction pathway.
- Rate constant
- Proportionality factor in a rate law.
- Reaction order
- Exponent describing concentration dependence in a rate law.
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