17. 1.28 g compound containing C, H and N is burned in pure oxygen producing 3.63 g CO2, 0.867 g H₂O and 0.192 g N₂. Calculate the empirical formula.C = 12.01 g/mole, H = 1.008 g/mole and N = 14.00 g/moleOOC6H7NO CHNC6HN5O C2H2N3

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17.1.28 g compound containing C, H and N is burned in pure oxygen producing 3.63 g CO₂, 0.867 g H₂O and 0.192 g N₂. Calculate the empirical formula. C = 12.01 g/mole, H = 1.008 g/mole and N = 14.00 g/mole O C6H7N OCHN O C6HN5 O C2H2N3

17.1.28 g compound containing C, H and N is burned in pure oxygen producing 3.63 g CO₂, 0.867 g H₂O and 0.192 g N₂. Calculate the empirical formula. C = 12.01 g/mole, H = 1.008 g/mole and N = 14.00 g/mole O C6H7N OCHN O C6HN5 O C2H2N3

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 93E

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Question

17. 1.28 g compound containing C, H and N is burned in pure oxygen producing 3.63 g CO2, 0.867 g H₂O and 0.192 g N₂. Calculate the empirical formula.
C = 12.01 g/mole, H = 1.008 g/mole and N = 14.00 g/mole
OO
C6H7N
O CHN
C6HN5
O C2H2N3

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