Theoretical Yield Calculator

Your details

Choose whether you know the mass or the moles of the limiting reactant.
The mass of the reactant that runs out first and caps product formation.
Sum the atomic masses of each element in the reactant formula (e.g. H2O = 2(1.008) + 15.999 = 18.015 g/mol).
g/mol
The number in front of the product in the balanced equation. For 2 H2 + O2 -> 2 H2O, the product H2O has coefficient 2.
The number in front of the limiting reactant in the balanced equation. For 2 H2 + O2 -> 2 H2O with H2 limiting, the coefficient is 2.
The molar mass of the product you want (e.g. 18.015 g/mol for water, 17.031 g/mol for ammonia).
g/mol
The unit used for the theoretical yield output.
Enable to enter the actual yield you recovered and calculate your percent yield.
Theoretical yield
36.03
Moles of product2mol
Moles of limiting reactant used2mol
Theoretical yield (g)36.03g
Theoretical yield (kg)0.03603kg
Theoretical yield (mg)36,030mg
Theoretical yield (lb)0.0794lb
Limiting reactant (mol)2
Product (mol)2

Theoretical yield: 36.03 g (2 mol of product)

  • The reaction can produce at most 36.03 g of product (2 mol). This ceiling is set entirely by the limiting reactant.
  • The limiting reactant runs out first. Any excess of other reactants remains unreacted and does not affect the theoretical yield.
  • Real reactions always produce less than the theoretical yield because of side reactions, handling losses, and equilibrium effects.

Next stepWeigh the product you recover, enter it as actual yield above, and enable "Calculate percent yield" to see your reaction efficiency.

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