If 23.7g of C8H18 are combusted, what mass of water will be produced?

Answer 1

First establish the combustion equation and have it balanced:
C₈H₁₈ + O₂ -> 8CO₂ + 9H₂O.
Balances for C, but not for O.
Since there are 16+9=25O on the right, we need to double the number to make the number of molecules on the left a whole number. So it becomes:
2C₈H₁₈ + 25O₂ -> 16CO₂ + 18H₂O.

Next step is to observe the relative molecular masses in ₈H₁₈ and 18H₂O.

You can then calculate the mass of H₂O produced by proportions using 23.7g of octane.

Answer 2

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