An unknown compound has the formula C HyO₂. You burn 0.2072 g of the compound and isolate 0.5059 g of CO2 and 0.2071 g of H₂O. What is the empirical formula of the compound? If the molar mass is 72.1 g/mol, what is the molecular formula? (Enter the elements in the order: C, H, O.) Empirical formula: Molecular formula:

An unknown compound has the formula C HyO₂. You burn 0.2072 g of the compound and isolate 0.5059 g of CO2 and 0.2071 g of H₂O. What is the empirical formula of the compound? If the molar mass is 72.1 g/mol, what is the molecular formula? (Enter the elements in the order: C, H, O.) Empirical formula: Molecular formula:

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter3: Equation, The Mole, And Chemical Formulas

Section: Chapter Questions

Problem 3.114QE

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

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An unknown compound has the formula C HyO₂. You burn
0.2072 g of the compound and isolate 0.5059 g of CO2 and
0.2071 g of H₂O. What is the empirical formula of the
compound? If the molar mass is 72.1 g/mol, what is the
molecular formula?
(Enter the elements in the order: C, H, O.)
Empirical formula:
Molecular formula:

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