13 notes ChemCalculations3_ppt [Compatibility Mode]

13 notes ChemCalculations3_ppt [Compatibility Mode] -...

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1 1 1 Lecture 13 Chemical Calculations, Chapter 9: Determining empirical and molecular formula from experiment data How can we determine, experimentally, the number of moles of each element that are present in a sample of an unknown pure compound? 2 Decomposition by Combustion s compounds containing only carbon and hydrogen burn in oxygen to produce CO 2 and H 2 O - calculate the mass and # moles of C from the mass of CO 2 - calculate the mass and # moles of H from the mass of H 2 O 3 Sample Calculation A sample of a pure substance containing only carbon and hydrogen weighs 1.025 g. When burned in oxygen, 3.007 g of CO 2 and 1.845 g of H 2 O were produced. What is the empirical formula of the sample compound? # moles of C in the sample compound = # moles of CO 2 produced # moles of H in the sample compound = 2 X # moles of H 2 O produced 4 Combustion Products: s The following compounds are produced from each of the listed elements when samples containing those elements are burned in oxygen C gives CO 2 H gives H 2 O N gives NO S gives SO 2
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13 notes ChemCalculations3_ppt [Compatibility Mode] -...

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