Theoretical Yield Calculator
Find the theoretical yield of a product from the moles of limiting reactant, mole ratio and molar mass.
How it works
theoretical yield (g) = moles of limiting reactant × mole ratio × product molar mass
The theoretical yield is the most product a reaction could possibly make if it went to completion with no losses. It is set entirely by the limiting reactant — the one that runs out first. Multiply its moles by the product-to-reactant mole ratio from the balanced equation, then by the product's molar mass, to convert to grams.
Worked example
With 0.5 mol of limiting reactant, a 1:1 mole ratio and a product of molar mass 58.44 g/mol (NaCl): 0.5 × 1 × 58.44 = 29.22 g theoretical yield.
Sources: Yield (chemistry) — Wikipedia
Frequently asked questions
What is the limiting reactant?
It is the reactant that is fully consumed first and therefore caps how much product can form. Any other reactant is in excess and left over at the end.
Where does the mole ratio come from?
From the coefficients of the balanced chemical equation. If 2 mol of reactant makes 3 mol of product, the product:reactant ratio is 3 ÷ 2 = 1.5.
How does this relate to percent yield?
Theoretical yield is the denominator of percent yield. Divide your actual measured yield by this value and multiply by 100 to get the percent yield.
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