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91: The rotten smell of a decaying animal carcass is partially due to a nitrogen-containing compound called putrescine. Elemental analysis of putrescine indicates that it consists of 54.50% C, 13.73% H, and 31.77% N. Calculate the empirical formula of putrescine. (Hint: Begin by assuming a 100-g sample and determining the mass of each element in that 100-g sample.)

91: The rotten smell of a decaying animal carcass is partially due to a nitrogen-containing compound called putrescine. Elemental analysis of putrescine indicates that it consists of 54.50% C, 13.73% H, and 31.77% N. Calculate the empirical formula of putrescine. (Hint: Begin by assuming a 100-g sample and determining the mass of each element in that 100-g sample.)

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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12:51 ( Search < Вack hw6.pdf 91: The rotten smell of a decaying animal carcass is partially due to a nitrogen-containing compound called putrescine. Elemental analysis of putrescine indicates that it consists of 54.50% C, 13.73% H, and 31.77% N. Calculate the empirical formula of putrescine. (Hint: Begin by assuming a 100-g sample and determining the mass of each element in that 100-g sample.) 95: A 1.45-g sample of phosphorous burns in air and forms 2.57 g of a phosphorous oxide. Calculate the empirical formula of the oxide. (Hint: Determine the mass of oxygen in the 2.57 g of phosphorous oxide by determining the difference in mass before and after the phosphorous burns in air.) 93: These compounds are found in many natural flavors and scents. Calculate the empirical formula for each compound Ethyl butyrate (pineapple oil): C 62.04%, H 10.41%, O 27.55% Methyl butyrate (apple flavor): C 58.80%, H 9.87%, O 31.33% Benzyl acetate (oil of jasmine): C 71.98%, H 6.71%, O 21.31% 101: The molar masses and empirical formulas of several compounds containing carbon and chlorine are listed here. Find the molecular formula of each compound 284.77 g/mol CCI, 131.39 g/mol C2HCI3, 181.44 g/mol C2HCI 103: A pure copper cube has an edge length of 1.42 cm. How many copper atoms does it contain? (volume of a cube = {edge length}3; density of copper = 8.96 g/cm3) Hint: Start by calculating the colume of the copper cube 105: A drop of water has a volume of approximately 0.05 mL. How many water molecules does it contain? (density of water = 1.0 g/cm³) 119: Butanedione, a compound in butter and body odor, has a cheesy smell. Elemental analysis of butanedione gave the mass percent composition: C 55.80%, H 7.03%, O 37.17%. The molar mass of butanedione is 86.09 g/mol. Determine the molecular formula of butanedione 121: Nicotine, a stimulant found in tobacco, has the mass percent composition: C 74.03%, H 8.70%, N 17.27%. The molar mass of nicotine is 162.26 g/mol. Find the molecular formula of nicotine, 127: An iron ore contains 38% Fe203 by mass. What is the maximum mass of iron that can be recovered from 10.0 kg of this one? ( Previous Next > 15 000 Dashboard Calendar Тo Do Notifications Inbox
Transcribed Image Text:12:51 ( Search < Вack hw6.pdf 91: The rotten smell of a decaying animal carcass is partially due to a nitrogen-containing compound called putrescine. Elemental analysis of putrescine indicates that it consists of 54.50% C, 13.73% H, and 31.77% N. Calculate the empirical formula of putrescine. (Hint: Begin by assuming a 100-g sample and determining the mass of each element in that 100-g sample.) 95: A 1.45-g sample of phosphorous burns in air and forms 2.57 g of a phosphorous oxide. Calculate the empirical formula of the oxide. (Hint: Determine the mass of oxygen in the 2.57 g of phosphorous oxide by determining the difference in mass before and after the phosphorous burns in air.) 93: These compounds are found in many natural flavors and scents. Calculate the empirical formula for each compound Ethyl butyrate (pineapple oil): C 62.04%, H 10.41%, O 27.55% Methyl butyrate (apple flavor): C 58.80%, H 9.87%, O 31.33% Benzyl acetate (oil of jasmine): C 71.98%, H 6.71%, O 21.31% 101: The molar masses and empirical formulas of several compounds containing carbon and chlorine are listed here. Find the molecular formula of each compound 284.77 g/mol CCI, 131.39 g/mol C2HCI3, 181.44 g/mol C2HCI 103: A pure copper cube has an edge length of 1.42 cm. How many copper atoms does it contain? (volume of a cube = {edge length}3; density of copper = 8.96 g/cm3) Hint: Start by calculating the colume of the copper cube 105: A drop of water has a volume of approximately 0.05 mL. How many water molecules does it contain? (density of water = 1.0 g/cm³) 119: Butanedione, a compound in butter and body odor, has a cheesy smell. Elemental analysis of butanedione gave the mass percent composition: C 55.80%, H 7.03%, O 37.17%. The molar mass of butanedione is 86.09 g/mol. Determine the molecular formula of butanedione 121: Nicotine, a stimulant found in tobacco, has the mass percent composition: C 74.03%, H 8.70%, N 17.27%. The molar mass of nicotine is 162.26 g/mol. Find the molecular formula of nicotine, 127: An iron ore contains 38% Fe203 by mass. What is the maximum mass of iron that can be recovered from 10.0 kg of this one? ( Previous Next > 15 000 Dashboard Calendar Тo Do Notifications Inbox
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