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Find the limiting reagent, theoretical yield, leftover excess reactants, and percent yield for any reaction, which is balanced for you first.
Also covers: Limiting reagent calculator ยท Theoretical yield calculator ยท Percent yield calculator ยท Mole ratio calculator
It's balanced for you. Use -> between sides and + between substances.
C3H8 + 5O2 โ 3CO2 + 4H2O
For percent yield.
Limiting reagent
O2
Theoretical yield of CO2: 105.628 g (2.40015 mol).
C3H8 + 5O2 โ 3CO2 + 4H2O
| Substance | M (g/mol) | Start (mol) | Reacts / forms (mol) | End (mol) | End (g) |
|---|---|---|---|---|---|
| C3H8 | 44.097 | 0.9978 | โ0.80005 | 0.19775 | 8.7202 |
| O2 | 31.998 | 4.0003 | โ4.0003 | 0 | 0 |
| CO2 | 44.009 | 0 | +2.4002 | 2.4002 | 105.63 |
| H2O | 18.015 | 0 | +3.2002 | 3.2002 | 57.652 |
Working
Type the equation; it doesn't need to be balanced, because it's balanced for you first.
Grams or moles for each reactant you know. Leave a reactant empty if it's in excess.
The limiting reagent, the theoretical yield of your chosen product, what's left of each reactant, and the percent yield if you enter the actual yield.
Each reactant's moles are divided by its coefficient in the balanced equation. The reactant with the smallest result runs out first, and it limits how much product can form.
The most product the limiting reagent can make if the reaction goes to completion with no losses. Percent yield = actual yield รท theoretical yield ร 100.
The others are assumed to be in excess, so that reactant is the limiting one.
No. Every calculation runs in your browser.
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