Combustion analysis of a compound yielded 236.73 g CO2, 48.48 g H2O, 61.86 g NO2, and 86.15 g SO2. (a) What is the empirical formula of the compound? (Assume it contains no oxygen.) (b) If the molar mass of the compound is 196.30 g/mol, what is the molecular formula of the compound?
Combustion analysis of a compound yielded 236.73 g CO2, 48.48 g H2O, 61.86 g NO2, and 86.15 g SO2. (a) What is the empirical formula of the compound? (Assume it contains no oxygen.) (b) If the molar mass of the compound is 196.30 g/mol, what is the molecular formula of the compound?
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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Combustion analysis of a compound yielded 236.73 g CO2, 48.48 g H2O, 61.86 g NO2, and 86.15 g SO2.
(a) What is the empirical formula of the compound? (Assume it contains no oxygen.)
(b) If the molar mass of the compound is 196.30 g/mol, what is the molecular formula of the compound?
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