An organic acid contains C, H, and O. In one combustion analysis, 5.24 g of acidyields 7.86 g CO2 and 2.14 g H2. Calculate the empirical formula and molecularformula of acid given that its molar mass is about 176 g/mol.A Empirical formula - CH „0 ;molecular formula - C,H1218Empirical formula - C H 0 ;molecular formula - C H20Empirical formula - CH 0 ; molecular formula - CH20,10Empirical formula -CH0, : molecular formula - CHO.

Mass of acid = 5.24 g Mass of CO2 = 7.86 g Mass of H2O = 2.14 g

s 7.86 g CO2 and 2.14 g H20. Calculate the empirical formula and molecular ula of acid given that its molar mass is about 176 g/mol. OEmpirical formula - CH,0 ; molecular formula - C H 1802 ) Empirical formula - C H 0 ; molecular formula - C Empirical formula - CH0 ;molecular formula - CH,e0 Empirical formula - C,H,0, : molecular formula - C HO. Н.о 6 8

s 7.86 g CO2 and 2.14 g H20. Calculate the empirical formula and molecular ula of acid given that its molar mass is about 176 g/mol. OEmpirical formula - CH,0 ; molecular formula - C H 1802 ) Empirical formula - C H 0 ; molecular formula - C Empirical formula - CH0 ;molecular formula - CH,e0 Empirical formula - C,H,0, : molecular formula - C HO. Н.о 6 8

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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