Use the following information to fill in the blanks below.Upon combustion, a 10.582 g sample of a C, H, O compound produced 26.976 g ofCO2 and 6.894 g of H20. The molar mass of the compound was determined to be483.28 g/mol.What is the mass of oxygen in the sample? Express your answer with threesignificant figures.What is the empirical formula? Do not worry about writing numbers as subscripts.What is the molecular formula? Do not worry about writing numbers as subscripts.

Sample Weight = 10.582 g CO = 226.9760 g H2O = 6.8940 gSample Weight g 10.582 Molar Weight of Sample g/mol 483.280 Moles of Sample mol 0.022 Flue Gas CO2 H2O Weight g 26.9760 6.8940 Molar Weight g/mol 44.0000 18.0000 Moles mol 0.6131 0.3830 Moles of C mol 0.6131 0.7660 No of Atoms mol 27.9999 34.9832 Atomic Mass of C g/mol 12.0000 Molar Mass from C g 335.9984 Atomic Mass of H g/mol 1.0000 Molar Mass from H g 34.9832 Molar Mass from C + H g 370.9816 Mass from O would be g 112.2984 Atomic Mass of O g/mol 16.0000 No of Atom O 7.0186 Mass of O in Sample would be g 2.4589 Empirical Formula C28.00 H34.98 O7.02 Molecular Formula C28 H35 O7

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Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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Use the following information to fill in the blanks below.
Upon combustion, a 10.582 g sample of a C, H, O compound produced 26.976 g of
CO2 and 6.894 g of H20. The molar mass of the compound was determined to be
483.28 g/mol.
What is the mass of oxygen in the sample? Express your answer with three
significant figures.
What is the empirical formula? Do not worry about writing numbers as subscripts.
What is the molecular formula? Do not worry about writing numbers as subscripts.

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