3D Activation Energy Simulation

Collisions, temperature, catalysts, and reaction rate

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Mission: give a molecule enough energy to cross the reaction barrier.

Temperature450 K

Activation energy60 kJ/mol

Relative concentration1.0×

Useful orientation60%

Add catalyst pathway

Reaction profile

Simulation speed1×

View

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Live measurements

Effective Ea60 kJ/mol

Fraction above Ea0.00%

Relative rate0.00

Successful collisions0 / s

k = A × e^(−Ea ÷ RT)

Lower energyAbove EaSuccessful collision

Energy and rate graph

Teacher tools

Show structure labels Reveal detailed explanation

Compare Cold and Hot without changing activation energy to isolate temperature.

Interactive complete lesson

Embedded audio controls the arrows, labels, camera, particles, and energy pathway.

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What is activation energy?

What to watch: A molecule climbs an energy hill only when it has enough kinetic energy.

Chapters

3D Activation Energy Simulation

Activation energy is the minimum energy needed for a collision to reach the transition state and produce a reaction.

Learning objectives

Identify reactants, products, transition state, and activation barrier.
Explain why many collisions do not form products.
Predict how temperature and concentration affect rate.
Explain orientation requirements and catalytic pathways.
Distinguish activation energy from overall energy change.

Key concepts demonstrated

Collision theory, kinetic-energy distributions, reaction coordinate, transition state, Arrhenius behavior, catalysts, orientation factor, concentration, and exothermic versus endothermic profiles.

Scientific equations

Arrhenius model: k = A × e^(−Ea ÷ RT). The energetic fraction is approximated by e^(−Ea ÷ RT). Here Ea is in joules per mole, R = 8.314 joules per mole-kelvin, and T is kelvin. The displayed rate is a normalized educational comparison.

Suggested experiments

Keep Ea fixed and compare 300 K with 700 K.
Switch the catalyst on without changing temperature.
Set orientation low, then rotate toward a useful collision.
Double concentration and watch collision frequency.

Questions for exploration

Why can a small temperature rise strongly increase rate?
Why does a catalyst not change the energy difference between reactants and products?
Can a high-energy collision still fail? Why?

Real-world applications

Enzymes, catalytic converters, food storage, combustion, industrial reactors, and medicine stability all depend on activation barriers and temperature.

Common misconceptions

A catalyst does not add energy; it supplies a lower-energy path.
Higher concentration does not lower Ea; it increases collision frequency.
Heating changes a distribution of energies, not one identical energy for every molecule.

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