Complete combustion of 8.50 g of a hydrocarbon produced 25.7 g of CO, and 13.2 g of H, 0. What is the empirical formula forthe hydrocarbon? Insert subscripts as necessary.empirical formula:CH An unknown compound contains only C, H, and O. Combustion of 4.80 g of this compound produced 11.7 g CO, and 4.80 gH,0. What is the empirical formula of the unknown compound? Insert subscripts as needed.empirical formula:CHO

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Answered: Complete combustion of 8.50 g of a…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter10: The Mole

Section: Chapter Questions

Problem 154A

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l-Dopa is a drug used for the treatment of Parkinson’s disease. Elemental analysis shows it to be 54.82% carbon, 7.10% nitrogen, 32.46% oxygen, and the remainder hydrogen. Determine l-dopa’s empirical formula. The molar mass of l-dopa is 197.19 g/mol. Determine its molecular formula.
A compound was analyzed and found to contain the following percentages of elements by mass: carbon, 79.89%; hydrogen, 20.11%. l type='a'> Determine the empirical formula of the compound. i>Which of the following could be a molar mass of the compound? 13.018 g/mol 16.042g/mol 28.052 g/mol 30.068 g/mol 104.23 g/rnol
What information do we need to determine the molecular formula of a compound from the empirical formula?
Tetrodotoxin is a toxic chemical found in fugu pufferfish, a popular but rare delicacy in Japan. This compound has an LD50 (the amount of substance that is lethal to 50.% of a population sample) of 10.g per kg of body mass. Tetrodotoxin is 41.38% carbon by mass, 13.16% nitrogen by mass, and 5.37% hydrogen by mass, with the remaining amount consisting of oxygen. What is the empirical formula of tetrodotoxin? If three molecules of tetrodotoxin have a mass of 1.59 1021 g, what is the molecular formula of tetrodotoxin? What number of molecules of tetrodotoxin would be the LD50 dosage for a person weighing 165 lb?
Uranium is used as a fuel, primarily in the form of uranium(IV) oxide, in nuclear power plants. This question considers some uranium chemistry. (a) A small sample of uranium metal (0.169 g) is heated to between 800 and 900 C in air to give 0.199 g of a dark green oxide, UxOy How many moles of uranium metal were used? What is the empirical formula of the oxide, UxOy? What is the name of the oxide? How many moles of UxOy must have been obtained? (b) The naturally occurring isotopes of uranium are 234U, 235U, and 238U. Knowing that uraniums atomic weight is 238.02 g/mol, which isotope must be the most abundant? (c) If the hydrated compound UO2(NO3)2 z H2O is heated gently, the water of hydration is lost. If you have 0.865 g of the hydrated compound and obtain 0.679 g of UO2(NO3)2 on heating, how many waters of hydration are in each formula unit of the original compound? (The oxide Ux, Oy is obtained if the hydrate is heated to temperatures over 800C in the air.)

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Complete combustion of 8.50 g of a hydrocarbon produced 25.7 g of CO, and 13.2 g of H, O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary. empirical formula: CH