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tombustion of a hrydrocarbon (C,H) sample produced 0.950 g of CO, and 0.130 g of H0. What is the empirical formula af the hydracarbon compound (what is x and what is y)? An unbalanced equation of the combustion reaction lyou do nat need to balance it) is CH,lg) + 0,(gl co,lg) +H,Olg) FMing in the blanks in the folowing sentences first may help you to answer the main question

tombustion of a hrydrocarbon (C,H) sample produced 0.950 g of CO, and 0.130 g of H0. What is the empirical formula af the hydracarbon compound (what is x and what is y)? An unbalanced equation of the combustion reaction lyou do nat need to balance it) is CH,lg) + 0,(gl co,lg) +H,Olg) FMing in the blanks in the folowing sentences first may help you to answer the main question

Introduction to Chemical Engineering Thermodynamics
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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vogsanb snpa Combustion of a hydrocarbon (C,H) sample produced 0.950 g of CO, and 0.13o g of H-0. What is the empirical formula of the hydrocarbon compound (what is x and what is y? An unbalanced equation of the combustion reaction lyou do nat need to balance it) is CH,Ig) + 0,(g)Co,(g) +H,0(g) FMing in the blonks in the foMowing sentences first may help you to answer the main question R is not required if it makes you more confused). There wif be no partial credit for this question. 0.950 g of CO, cOIrespond to moles of COz. 0.130 g of H-DcNTespond to moles of HA. Each molecule of CO, came from Catom(s) in C,H, Each mole of C0,come from molefs) of C in C,H, How many moles of C were there in C,H,? Each molecule of H-O come from Hotom(s) in CA, Each mole of HOcome from mole(s) of H in C,H, How many moles of H were there in CH,? Now you are on your owmI. OL CH, OE CH OD CH OL CH,.
Transcribed Image Text:vogsanb snpa Combustion of a hydrocarbon (C,H) sample produced 0.950 g of CO, and 0.13o g of H-0. What is the empirical formula of the hydrocarbon compound (what is x and what is y? An unbalanced equation of the combustion reaction lyou do nat need to balance it) is CH,Ig) + 0,(g)Co,(g) +H,0(g) FMing in the blonks in the foMowing sentences first may help you to answer the main question R is not required if it makes you more confused). There wif be no partial credit for this question. 0.950 g of CO, cOIrespond to moles of COz. 0.130 g of H-DcNTespond to moles of HA. Each molecule of CO, came from Catom(s) in C,H, Each mole of C0,come from molefs) of C in C,H, How many moles of C were there in C,H,? Each molecule of H-O come from Hotom(s) in CA, Each mole of HOcome from mole(s) of H in C,H, How many moles of H were there in CH,? Now you are on your owmI. OL CH, OE CH OD CH OL CH,.
Expert Solution
Step 1

Given 

weight of CO2 formed=0.95 g

moles of CO2 formed=0.9544=0.0216 moles

weight of H2O formed=0.13 g

moles of H2O formed=0.1318=0.00722 moles

Reaction:

CxHy+(2x+y22)O2→xCO2+ y2H2O

 

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