Rate of reaction
High School
Definition
A measure of how quickly reactants are converted into products, often expressed as the change in concentration over time. The rate is influenced by temperature, concentration, surface area, and catalysts.
Worked examples
\(\)Rate\( = \frac{\Delta[\)Product\(]}{\Delta t}\)
Rate equals the change in product concentration divided by the change in time.
Marble chips react faster with acid than a single marble block of the same mass.
Greater surface area increases the rate by exposing more reactant particles to collision.
Hydrogen peroxide decomposes slowly at room temperature but rapidly with manganese dioxide catalyst.
A catalyst speeds up the reaction without being consumed.
Common mistakes
- Higher concentration always means the reaction finishes sooner. → Higher concentration increases the rate, but total time also depends on the amount of reactant. Rate and total reaction time are related but not the same thing.
- Catalysts increase the yield of product. → Catalysts increase the rate but do not change the equilibrium yield. Catalysts speed up how fast equilibrium is reached, not how much product forms.
- Cooling a reaction increases its rate because particles move less chaotically. → Cooling decreases the rate because particles have less kinetic energy and collide less often. Lower temperature means fewer effective collisions per unit time.
Where you'll use it next
Rate of reaction is essential for chemical equilibrium, enzyme kinetics in biology, industrial process optimization, and understanding reaction mechanisms in advanced chemistry.
Found in 1 StudyPug lesson
Understanding Factors Affecting Rate of Reaction
12th Grade12thChemistry 12
Dive into the world of chemical kinetics and discover how temperature, concentration, surface area, and catalysts influence reaction rates. Master these concepts to excel in chemistry and real-world applications.
See also
Reviewed by Pat Cheng, M.Ed. — StudyPug Curriculum Lead · Last updated June 6, 2026