How to find Excess Reactant and Limiting Reactant

Limiting Reactant:

“The reactant which is earlier consumed in a chemical reaction” is called limiting reactant.


   “The reactant which is completely consumed in a reaction to produce product when the reaction is over” is called limiting reactant.

Limiting reactant is also known as limiting reagent.

Excess Reactant:

The substance whose some amount is left unreacted when the reaction is over is called substance in excess.


The reactant which is not used up completely and its some amount remains unused after the chemical reaction is termed as excess reactant.

Excess reactant is also known as excess reagent.

 Determining the Limiting reactant and Excess Reactant:

Consider a chemical reaction ( irreversible reaction) :

e.g.      Let 4 moles of nitrogen are made to react with 6 moles of hydrogen to get ammonia.

N2(g)    +   3H2(g)  → 2NH3(g)

Molar ratio according to equation       1 mole             3 moles                             2 moles

Suppose 4 moles of N2 and 6 moles of H2 are made to react, then

Moles present before reaction             4 moles             6 moles                                  0 mole

Moles present after reaction                2 moles            0 mole                                    4 moles

                                                         ( excess reactant )    (Limiting reactant)

As H2 is consumed completely so it is limiting reactant while 2 moles of N2 are left unreacted so it is substance in excess. Thus product will be calculated by H2 which is the limiting reactant.

  • In a balanced chemical equation, no reactant is limiting or in excess.
  • Consider a chemical reaction

    2H2(g)      +    O2(g) → 2H2O(g)

    Formation of water (2H2O) is a balanced chemical equation .Therefore, no reactant is limiting or in excess.

    However, when 1mole of each H2 and O2 react together ,then they form a chemical equation:

    2 mol H2 gives = 2 mol H2O

    1 mol H2 gives = 2/2 mol H2O

    1 mol H2 gives = 1 mol H2O

    Similarly :

    1 mol O2 gives = 2 mol H2O

    As one mole of hydrogen (H2) gives the least amount of product ( 1 mole of H2O).

    Hence , H2 is a limiting reactant while O2 is an excess reactant .

    Also Read !!!

    Mole and Avogadro’s Number | Important Questions

    Stoichiometry Important Terms Definitions

    Mole and Chemical Equation

    What is the difference between Octet Rule and Duplet Rule

    Basic Atomic Structure

    What is the difference between Shell , Subshell and Orbital

    How ions are formed (Cation vs Anion)

    Ionic Bond : Definition, Examples & Formation

    Covalent Bond :Definition and Examples

    Get in touch !!

    Visit & Follow me !!

    Leave a Reply

    Fill in your details below or click an icon to log in: Logo

    You are commenting using your account. Log Out /  Change )

    Google photo

    You are commenting using your Google account. Log Out /  Change )

    Twitter picture

    You are commenting using your Twitter account. Log Out /  Change )

    Facebook photo

    You are commenting using your Facebook account. Log Out /  Change )

    Connecting to %s