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Liquid octane reacts with gaseous oxygen gas to produce gaseous carbon dioxide and gaseous water . if 55.0 g of water is produced from the reaction of 99.37 g of octane and 668.1 g of oxygen gas, calculate the percent yield of water. round your answer to 3 significant figures.
Accepted Answer
Here's how to calculate the percent yield of water:
1. Write the balanced chemical equation:
C8H18(l) + 12.5O2(g) → 8CO2(g) + 9H2O(g)
2. Calculate the theoretical yield of water:
- Convert grams of octane to moles: 99.37 g C8H18 / 114.23 g/mol = 0.870 mol C8H18
- Use the mole ratio from the balanced equation to find moles of water: 0.870 mol C8H18
(9 mol H2O / 1 mol C8H18) = 7.83 mol H2O
- Convert moles of water to grams: 7.83 mol H2O
18.02 g/mol = 141 g H2O
3. Calculate the percent yield:
- Percent yield = (actual yield / theoretical yield)
100%
- Percent yield = (55.0 g / 141 g)
100% = 39.0%
Therefore, the percent yield of water is 39.0%.
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