What does the Arrhenius equation explain?
Why reactions go faster when heated. Because temperature sits in an exponent, even a small rise gives a big jump in rate - roughly doubling for every 10°C.
// chemistry › Temperature Dependence
Arrhenius Equation
Compute the rate constant k = A·e^(−E_a/RT), with symbol legend and real-world examples.
k = A\,e⁻Eₐ / (R\,T)
A mind behind this: Svante Arrhenius 1859–1927
Frequently asked questions
What is activation energy?
The energy 'hill' molecules must climb to react. A high hill means few make it over (slow); a low hill means many do (fast). Catalysts lower the hill.
Why does temperature have such a big effect?
Because it sets the fraction of molecules with enough energy to clear the hill, and that fraction rises exponentially with temperature - so the rate climbs steeply, not linearly.
How do catalysts fit in?
They give a lower-energy path - a smaller hill - so k rises dramatically without adding heat, and the catalyst is not used up. Enzymes do this in your body.
What are A and R?
A is how often molecules collide with the right orientation (the top possible rate). R is the gas constant (8.314 J/mol·K) that keeps the units consistent in the exponent.