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3.12a Empirical formula of a compound containing sulfur and oxygen

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Chimie

Université du Kentucky

4.7 (664 notes) | 67K étudiants inscrits

This course is designed to cover subjects in advanced high school chemistry courses, correlating to the standard topics as established by the American Chemical Society. This course is a precursor to the Advanced Chemistry Coursera course. Areas that are covered include atomic structure, periodic trends, compounds, reactions and stoichiometry, bonding, and thermochemistry.

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4.7 (664 notes)

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À partir de la leçon

Week 3

Now that we know the structure of an atom, we can explore how atoms combine to form either molecular or ionic compounds. Then we will learn the rules of nomenclature that ensure that a compound is named according to IUPAC rules. We will end this unit by looking at quantitative relationships for compounds including the molar mass of and mass percent of an element in a compound.

3.01 Elements vs. Compounds 14:40

3.02 Types of Chemical Bonds 7:25

3.03 Chemical Formulas 7:37

3.04 Formula of ionic compounds 12:46

3.04a Formula of the compound formed from aluminum and phosphorus 1:19

3.04b Formula of the compound formed from ammonium and phosphate 1:27

3.05 Nomenclature 6:26

3.06 Nomenclature of Ionic Compounds 10:42

3.06a IUPAC Name for K2SO4 0:57

3.06b IUPAC Name for NiCO3 1:54

3.06c Formula for manganese(II) flouride 0:52

3.06d IUPAC Name for AgNO3 1:04

3.06e Formula for chromium(III) oxide 1:00

3.07 Nomenclature of Molecular Compounds 8:41

3.07a IUPAC Name for PCl3 1:21

3.07b IUPAC Name for N2O1:01

3.07c Formula for boron triflouride 0:40

3.08 Nomenclature of Acids 5:54

3.09 Molar Mass of Compounds 11:41

3.09a Molecular Mass of Al2(Cr2O7)31:47

3.09b Mass of a sample of vitamin C 2:39

3.09c Moles of sucrose within a sugar cube 2:03

3.10 Mass percent composition 8:55

3.10a Mass percent of chromium 1:53

3.10b Mass of CaCl2 containing chlorine 2:29

3.11 Relationships from Chemical Formulas 11:39

3.11a Mass of H in Ca(H2PO4)2 3:30

3.11b Mass of NH3 2:13

3.12 Chemical formulas from experimental data 9:46

3.12a Empirical formula of a compound containing sulfur and oxygen 2:13

Enseigné par

Dr. Allison Soult
Lecturer
Dr. Kim Woodrum
Sr. Lecturer

Transcription

We have a mass that has 83.5 grams, containing only sulfur and oxygen and we're given the mass of the sulfur. And so what we want to find is the empirical formula? So, if we know it's only sulfur and oxygen, if it's not sulfur, the rest of the mass must be oxygen. So we can actually find the mass of the oxygen by subtracting 83.5 grams of compound, minus our 33.4 grams of sulfur, and we end up having 50.1 grams of oxygen. So, when we're trying to find empirical formulas, what we've got to find is the molar ratio between the elements in that compound. So, we're going to look at our sulfur first. We know we have 33.4 grams of sulfur, and I want to get that into moles. And our molar mass of sulfur is 32.0 grams per mole, and what that gives me is 1.04 moles of sulfur. I'm going to do the same thing for my oxygen, but I have 50.1 grams of oxygen, and my mass of oxygen is 16.0 grams per mole, and that gives me 3.13 moles of oxygen. Now, I can actually look at these ratios and figure out what the formula is. I don't want to leave it as sulfur 1.04, oxygen 3.13. We want nice integers for our subscripts. So, what we want to do is actually divide by the lowest number of moles. In this case, it's going to be the 1.04, and I'm going to divide each of those values by that same number, and what I get is a 1 for the sulfur and a 3 for the oxygen. And so, I can now write my empirical formula because I get sulfur 1, which we're not going to put the subscript in, O3. So, that shows me the molar ratio between the sulfur and the oxygen, and it leaves me with whole number integers for my subscripts.

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