Question 95. 12:51( Search< Вackhw6.pdf91: The rotten smell of a decaying animal carcass is partially due to a nitrogen-containingcompound called putrescine. Elemental analysis of putrescine indicates that it consists of54.50% 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-gsample.)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 the2.57 g of phosphorous oxide by determining the difference in mass before and after thephosphorous burns in air.)93: These compounds are found in many natural flavors and scents. Calculate the empiricalformula for each compoundEthyl 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 andchlorine are listed here. Find the molecular formula of each compound284.77 g/mol CCI, 131.39 g/mol C2HCI3, 181.44 g/mol C2HCI103: A pure copper cube has an edge length of 1.42 cm. How many copper atoms does itcontain? (volume of a cube = {edge length}3; density of copper = 8.96 g/cm3) Hint: Start bycalculating the colume of the copper cube105: A drop of water has a volume of approximately 0.05 mL. How many water moleculesdoes it contain? (density of water = 1.0 g/cm³)119: Butanedione, a compound in butter and body odor, has a cheesy smell. Elementalanalysis 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 ofbutanedione121: Nicotine, a stimulant found in tobacco, has the mass percent composition: C 74.03%, H8.70%, N 17.27%. The molar mass of nicotine is 162.26 g/mol. Find the molecular formula ofnicotine,127: An iron ore contains 38% Fe203 by mass. What is the maximum mass of iron that canbe recovered from 10.0 kg of this one?( PreviousNext >15000DashboardCalendarТo DoNotificationsInbox

When phosphorus burns in the air, it absorbs oxygen gas which results in the formation of oxide. The…

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.)

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.)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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