EasyChemistryHigh School (11–12)Atoms and Molecules › Stoichiometry and ConcentrationAtoms and Molecules › The Mole ConceptNumerical
A lighter holds butane, which burns as 2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O.
Contributed by StemPy LabTry it on paper first. A hint, the key idea and the worked solution are here when you need them.
A lighter holds butane, which burns as . How many grams of oxygen does of butane use, and how many grams of carbon dioxide does it make? Butane is .
Need a reminder? The key ideaShow
The coefficients of a balanced equation give the mole ratio. Mass to moles, moles by the mole ratio, then moles to mass. At STP one mole of a gas fills . The limiting reagent has the smallest moles divided by its coefficient; it is used up and fixes the product.
The worked solution
Have you tried it?
Work it out on paper first. It is fine to get stuck or make a mistake: that is how we learn. When you are ready, go through the solution one step at a time, and check each step against your own.
Step 1. Butane. .
Step 2. Oxygen. , which is .
Step 3. Carbon dioxide. , which is .
Answer: of oxygen, and of carbon dioxide.
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