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

  • Chemistry -

    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.

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