Difference between revisions of "Limiting reactant"
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Say you have equimolar quantities of [[hydrogen]] (H<sub>2</sub>) and [[oxygen]] (O<sub>2</sub>). Since 2 [[mole]]s of hydrogen are required for every 1 mole of oxygen, when all the hydrogen is used up there is still leftover oxygen. Thus, hydrogen is the limiting reactant, because it is used up first. | Say you have equimolar quantities of [[hydrogen]] (H<sub>2</sub>) and [[oxygen]] (O<sub>2</sub>). Since 2 [[mole]]s of hydrogen are required for every 1 mole of oxygen, when all the hydrogen is used up there is still leftover oxygen. Thus, hydrogen is the limiting reactant, because it is used up first. | ||
| − | ==See | + | ==See also== |
*[[Rate limiting step]] | *[[Rate limiting step]] | ||
[[Category:Chemistry]] | [[Category:Chemistry]] | ||
Latest revision as of 15:22, July 13, 2016
In a chemical reaction, the limiting reactant is the species which is in lowest stoichiometric quantity. In other words, it is the reactant which is consumed before any others.
Example
Take the chemical reaction
- <math>2H_2 + O_2 \rightarrow 2H_2O</math>.
Say you have equimolar quantities of hydrogen (H2) and oxygen (O2). Since 2 moles of hydrogen are required for every 1 mole of oxygen, when all the hydrogen is used up there is still leftover oxygen. Thus, hydrogen is the limiting reactant, because it is used up first.