Enter a fuel (e.g. C3H8, C2H6O) and we'll fill in + O2 → CO2 + H2O for you, then balance it.
Examples:
CombustionA fuel reacts with O₂ to produce CO₂ and/or H₂O.
CH4+2O2→CO2+2H2O
Yield analysis
Amounts in
Enter how much of each reactant you have. The limiting reagent, theoretical yield of each product, and (if you fill in an actual yield) percent yield appear automatically.
Reactants
| CH4×1 | ||
| O2×2 |
Products — theoretical & actual
| Species | Theoretical | Actual (g) | % yield |
|---|---|---|---|
| CO2 | — | — | |
| H2O | — | — |
| Species | Coefficient | Molar mass (g/mol) |
|---|---|---|
| CH4reactant | 1 | 16.042 |
| O2reactant | 2 | 32.000 |
| CO2product | 1 | 44.010 |
| H2Oproduct | 2 | 18.016 |