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Liquid octane reacts with gaseous oxygen gas to produce gaseous carbon dioxide and gaseous water . if 3.75 g of water is produced from the reaction of 8.00 g of octane and 47.0 of oxygen gas, calculate the percent yield of water. round your answer to 3 significant figures. What is the answer?
Accepted Answer
Here's how to calculate the percent yield of water in this reaction:
1. Write the balanced chemical equation:
C8H18 (l) + 25/2 O2 (g) → 8 CO2 (g) + 9 H2O (g)
2. Calculate the theoretical yield of water:
Convert the mass of octane (8.00 g) to moles using its molar mass (114.23 g/mol):
8.00 g C8H18 × (1 mol C8H18 / 114.23 g C8H18) = 0.0700 mol C8H18
Use the mole ratio from the balanced equation to find the moles of water produced:
0.0700 mol C8H18 × (9 mol H2O / 1 mol C8H18) = 0.630 mol H2O
Convert the moles of water to grams using its molar mass (18.015 g/mol):
0.630 mol H2O × (18.015 g H2O / 1 mol H2O) = 11.3 g H2O (theoretical yield)
3. Calculate the percent yield:
Percent yield = (actual yield / theoretical yield) × 100%
Percent yield = (3.75 g H2O / 11.3 g H2O) × 100%
Percent yield = 33.2%
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