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reaction rate
Sign in to saveAlso known as speed of reaction, rate of reaction
for a reactant or product in a particular reaction is intuitively defined as how quickly or slowly a reaction takes place
In the Vinony graph
Vinony's link graph records 267 inbound references to reaction rate, and connects out to rate equation, International Union of Pure and Applied Chemistry and stoichiometry.
It sits within the topics Chemical kinetics, Chemical reaction engineering and Temporal rates.
Vinony links it to 48 Wikipedia language editions.
Key facts
- Common symbols
- ν
- Other units
- mol ⋅ L ⋅ s
- In si base units
- mol ⋅ m ⋅ s
- Dimension
- L ⋅ T ⋅ N
via Wikipedia infobox
Wikidata facts
- Instance of
- chemical property
- Subclass of
- physical quantity
- Image
- Large bonfire.jpg
Show 2 more facts
- studied by
- chemical kinetics
- maintained by WikiProject
- WikiProject Mathematics
Sources (3)
via Wikidata · CC0
~20 min read
Encyclopedic overview
Iron rusting has a low reaction rate. This process is slow. Wood combustion has a high reaction rate. This process is fast.
The reaction rate or rate of reaction is the speed at which a chemical reaction takes place, defined as proportional to the increase in the concentration of a product per unit time and to the decrease in the concentration of a reactant per unit time. Reaction rates can vary dramatically. For example, the oxidative rusting of iron under Earth's atmosphere is a slow reaction that can take many years, but the combustion of cellulose in a fire is a reaction that takes place in fractions of a second. For most reactions, the rate decreases as the reaction proceeds. A reaction's rate can be determined by measuring the changes in concentration over time.
Excerpted from Wikipedia’s “reaction rate” article, available under the CC BY-SA 4.0 licence.