Advertisements
Advertisements
Question
What is a limiting reagent? Explain.
Solution
- The reactant which gets consumed and limits the amount of product formed is called the limiting reagent.
- When a chemist carries out a reaction, the reactants are not usually present in exact stoichiometric amounts, that is, in the proportions indicated by the balanced equation.
- This is because the goal of a reaction is to produce the maximum quantity of a useful compound from the starting materials. Frequently, a large excess of one reactant is supplied to ensure that the more expensive reactant is completely converted into the desired product.
- The reactant which is present in a lesser amount gets consumed after some time and subsequently, no further reaction takes place, whatever be the amount left of the other reactant present.
Hence, limiting reagent is the reactant that gets consumed entirely and limits the reaction.
APPEARS IN
RELATED QUESTIONS
In a reaction, \[\ce{A + B2 -> AB2}\]
Identify the limiting reagent, if any, in the following reaction mixture.
300 atoms of A + 200 molecules of B
In a reaction, \[\ce{A + B2 -> AB2}\]
Identify the limiting reagent, if any, in the following reaction mixture.
2 mol A + 3 mol B
In a reaction, \[\ce{A + B2 -> AB2}\]
Identify the limiting reagent, if any, in the following reaction mixture.
100 atoms of A + 100 molecules of B
In a reaction, \[\ce{A + B2 -> AB2}\]
Identify the limiting reagent, if any, in the following reaction mixture.
5 mol A + 2.5 mol B
In a reaction, \[\ce{A + B2 -> AB2}\]
Identify the limiting reagent, if any, in the following reaction mixture.
2.5 mol A + 5 mol B
Explain the term molarity
The reactant which is entirely consumed in reaction is known as limiting reagent. In the reaction \[\ce{2A + 4B -> 3C + 4D}\], when 5 moles of A react with 6 moles of B, then which is the limiting reagent?
The reactant which is entirely consumed in reaction is known as limiting reagent. In the reaction \[\ce{2A + 4B -> 3C + 4D}\], when 5 moles of A react with 6 moles of B, then calculate the amount of C formed?
Calcium carbonate reacts with aqueous \[\ce{HCl}\] to give \[\ce{CaCl2}\] and \[\ce{CO2}\] according to the reaction given below:
\[\ce{CaCO3(s) + 2HCl (aq) -> CaCl2 (aq) + CO2(g) + H2O (l)}\]
What mass of \[\ce{CaCl2}\] will be formed when 250 mL of 0.76 M \[\ce{HCl}\] reacts with 1000 g of \[\ce{CaCO3}\]? Name the limiting reagent. Calculate the number of moles of \[\ce{CaCl2}\] formed in the reaction.
