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What is the empirical formula of a compound containing C, H, and O if combustion of 1.23 g of the compound yields 1.8 g CO2 and 0.

What is the empirical formula of a compound containing C, H, and O if combustion of 1.23 g of the compound yields 1.8 g CO2 and 0.74 g H2O

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  • moles of C present = 0.49gC/12.01g =0.041 mol C ; moles of H present = 0.083g H/ 1.008gH= 0.082 mols ; moles of O present = 0.657gO/16.00gO = 0.041 moles ; therefore we find the ratio of C, H and O present in the compound by dividing each moles by the smallest number of the moles in this case, 0.041 is the smallest and therefore the ratio is = 1 : 2 : 1 respectively ; therefore the empirical formula of the compound is CH2O.
    • okiyaiomuse
    • May 06, 2018 at 6:20am
  • am sorry i posted the answer by mistake when it was incomplete.....
    • okiyaiomuse
    • May 06, 2018 at 6:22am

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