Textbook Question
From the given empirical formula and molar mass, find the molecular formula of each compound. a. C6H7N, 186.24 g/mol
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Ch.3 - Molecules, Compounds & Chemical Equations
Chapter 3, Problem 96c
From the given molar mass and empirical formula of several compounds, find the molecular formula of each compound. c. C3H2N, 312.29 g/mol
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Empirical Formula
The empirical formula represents the simplest whole-number ratio of atoms of each element in a compound. It provides essential information about the composition of the compound but does not indicate the actual number of atoms present. For example, the empirical formula for glucose (C6H12O6) is CH2O, which shows the ratio of carbon, hydrogen, and oxygen.
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02:26
Empirical vs Molecular Formula
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms in the molecular formula. In the context of finding a molecular formula, the molar mass helps determine how many times the empirical formula fits into the molecular formula based on the given total mass.
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02:11Molar Mass Concept
Molecular Formula
The molecular formula indicates the actual number of atoms of each element in a molecule of a compound. It can be derived from the empirical formula by multiplying the subscripts in the empirical formula by a whole number, which is determined by dividing the compound's molar mass by the molar mass of the empirical formula. This provides a complete picture of the compound's composition.
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02:08Determining Molecular Formulas
Related Practice
Textbook Question
From the given molar mass and empirical formula of several compounds, find the molecular formula of each compound. a. C4H9, 114.22 g/mol
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Textbook Question
From the given molar mass and empirical formula of several compounds, find the molecular formula of each compound. b. CCl, 284.77 g/mol
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Textbook Question
Combustion analysis of a hydrocarbon produces 33.01 g CO2 and 13.51 g H2O. Calculate the empirical formula of the hydrocarbon.
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Textbook Question
Combustion analysis of naphthalene, a hydrocarbon used in mothballs, produces 8.80 g CO2 and 1.44 g H2O. Calculate the empirical formula of naphthalene.
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Textbook Question
The foul odor of rancid butter is due largely to butyric acid, a compound containing carbon, hydrogen, and oxygen. Combustion analysis of a 4.30-g sample of butyric acid produces 8.59 g CO2 and 3.52 g H2O. Determine the empirical formula of butyric acid.
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