Class 12 Chemistry simulations · Chemical Kinetics

Arrhenius equation and activation energy

Change the temperature and activation energy and see how many molecules have enough energy to react.

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What to notice

A 10 K rise near room temperature roughly doubles the rate for Eₐ ≈ 50 kJ/mol, because many more molecules cross the barrier.

Key relation

k = A e^(−Eₐ/RT) ; log(k₂/k₁) = Eₐ/(2.303R) · (1/T₁ − 1/T₂)

Try this

Set Eₐ = 50 kJ/mol and compare 298 K with 308 K.

What you can change

• Activation energy Eₐ: 10 to 150 kJ/mol
• Temperature: 250 to 500 K

More in Chemical Kinetics

• How a catalyst speeds up a reaction
• Order of reaction and half-life

See all Class 12 Chemistry simulations or every Physica simulation.