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A 6.67 mg sample of a compound containing carbon, hydrogen, and oxygen underwent combustion producing 15.17 mg of CO2 and 6.19 mg of H2O. What is the empirical formula of the compound? (Type your answer using the format CxHyOz for the compound CxHyOz)

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mickymike92

The empirical formula of the compound is C₃H₆O

What is the empirical formula of the compound?

The empirical formula is determined as follows from the equation of the reaction as follows:

  • CxHyOz + O₂ → x CO₂ + y/z H₂O

mass of CO₂ produced = 15.17 mg = 0.01517 g

moles of C in the sample = 0.01517/44  = 0.000344 moles

mass of C in the sample =  0.0000344  * 12 = 0.00413 g

mass of H₂O produced  = 6.19 mg = 0.00619 g

moles of H in the sample = 0.00619/18 * 2 = 0.000688 moles

mass of H in sample = 0.000688 g

mass of oxygen in the sample = 0.00667 g - (0.00413 g + 0.000688 g)

mass of oxygen in the sample = 0.00185

moles of oxygen = 0.00185/16 = 0.000116

Ratio of C : H : O = 0.000344 : 0.000688 : 0.000116

Ratio of C : H : O = 3 : 6 : 1

Empirical formula of compound = C₃H₆O

Learn more about empirical formula at: https://brainly.com/question/13058832

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