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empirical formulas

# empirical formulas - 0.3576 = 1.000 mol C 0.7154 mol H...

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Feedback: Please note that while the results of the intermediate calculations below are displayed rounded to 4 significant figures, the actual calculations are done internally without rounding. Step 1. Use the masses of CO 2 and H 2 O produced to calculate the moles of H and C present in the original sample. Note that there are 2 mol H per mol H 2 O. 15.74 g CO 2 1 mol CO 2 1 mol C = 0.3576 mol C 44.01 g 1 mol CO 2 6.446 g H 2 O 1 mol H 2 O 2 mol H = 0.7154 mol H 18.02 g 1 mol H 2 O Step 2. Determine integer mole ratios and the empirical formula. Multiplying or dividing both quantities by the same number will not change the relative number of moles. Begin by dividing both quantities by the smallest number of moles calculated in Step 1. 0.3576 mol C /

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Unformatted text preview: 0.3576 = 1.000 mol C 0.7154 mol H / 0.3576 = 2.000 mol H These numbers are close enough to integer values to be rounded to integers. 1.000 mol C = 1 mol C 2.000 mol H = 2 mol H EMPIRICAL FORMULA = CH 2 . Step 3. Determine the molecular formula for the compound. Divide the molar mass of the compound ( 28.05 g/mol) by the empirical formula weight to determine the number of empirical units in the molecule. Empirical weight for CH 2 = 1 ( 12.01 ) + 2 ( 1.008 ) = 14.03 g/mol empirical unit Molecular Weight = 28.05 g/mol molecule = 2.00 empirical units / molecule Empirical Weight 14.03 g /mol empirical unit There are 2 CH 2 units per molecule. MOLECULAR FORMULA = ( CH 2 ) 2 = C 2 H 4...
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empirical formulas - 0.3576 = 1.000 mol C 0.7154 mol H...

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