Combustion analysis of a compound yielded 235.50 g CO2, 72.33 g H2O, 61.57 g NO2, and...

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Combustion analysis of a compound yielded 235.50 g CO2, 72.33 gH2O, 61.57 g NO2, and 85.72 g SO2. (a) What is the empiricalformula of the compound? (Assume it contains no oxygen.) chemPadHelp C2H2NO Your answer appears to substitute one element foranother. (b) If the molar mass of the compound is 200.34 g/mol,what is the molecular formula of the compound?

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Number of moles of CO2 n massmolar mass 23550 g 44gmol 535 moles So number of moles of C is 535 mol Number of moles of H2O is n massmolar mass See Answer

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Combustion analysis of a compound yielded 235.50 g CO2, 72.33 g H2O, 61.57 g NO2, and...

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Chemistry

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