A major component of gasoline is octane (C₈H₈). When octane is burned in air, it chemically reacts with oxygen gas (O₂) to produce carbon dioxide (CO₂) and water (H₂O) .
What mass of octane is consumed by the reaction of 3.1 g of oxygen gas?
The balanced equation is
2 C8H18 + 25 O2 -----> 16 CO2 + 18 H2O
Number of moles of O2 = 3.1g / 32.0 g/mol = 0.0969 mole
from the balanced equation we can say that
25 mole of O2 requires 2 mole of octane so
0.0969 mol of O2 will require
= 0.0969 mol of O2 *(2 mole of octane / 25 mole of O2)
= 0.00775 mole of octane
mass of 1 mole of octane = 114.23 g
so the mass of 0.00775 mole of octane = 0.89 g
Therefore, the mass of octane consumed = 0.89 g
What mass of octane is consumed by the reaction of 3.1 g of oxygen gas?
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