'Empirical formula mass' diaporamas de présentation

The Mole and Stoichiometry

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Stoichiometry 1 Formulas and the Mole

Stoichiometry 1 Formulas and the Mole. L. Scheffler Lincoln High School. 1. The Mole. Chemical reactions involve atoms and molecules. The ratios with which elements combine depend on the number of atoms not on their mass. The masses of atoms or molecules depend on the substance.

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Stoichiometry 1 Formulas and the Mole

Stoichiometry 1 Formulas and the Mole. L. Scheffler Lincoln High School. 1. The Mole. Chemical reactions involve atoms and molecules. The ratios with which elements combine depend on the number of atoms not on their mass. The masses of atoms or molecules depend on the substance.

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Chapter 7 Chemical Quantities

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Section 4: Empirical and Molecular Formulas

Section 4: Empirical and Molecular Formulas. Chemical Composition. Learning Goals. Explain what is meant by the percent composition of a compound. Determine the empirical and molecular formulas for a compound from mass percent and actual mass data. Percent Composition.

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Writing Empirical and Molecular Formulas

Writing Empirical and Molecular Formulas. What is an empirical formula?. A chemical formula in which the ratio of the elements are in the lowest terms is called an empirical formula . . Example:.

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Chapter 7 Chemical Quantities

Chapter 7 Chemical Quantities. Fall 2008. The Mole: A Measurement of Matter-What Is a Mole?. How do you measure matter? You count things You weigh things or determine mass You get the volume Can you count the grains of sand? Would you want to?

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Chapter 7 Section 3 and 4

Chapter 7 Section 3 and 4. Percent composition Empirical Formula Molecular Formula. Calculating Formula Mass. Calculate the formula mass of magnesium carbonate, MgCO 3 . 24.31 g + 12.01 g + 3(16.00 g) =. 84.32 g. Calculating Percentage Composition.

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Chemical Equations

Chemical Equations. p.13 Q1 Write balanced equations including state symbols for the following: (a) zinc + oxygen ? zinc oxide 2 Zn (s) + O 2 (g) ? 2 ZnO (s) (b) potassium + water ? potassium hydroxide + hydrogen 2 K (s) + 2 H 2 O (l) ? 2 KOH (aq) + H 2 (g)

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Chapter 3

Chapter 3. Molecules, Compounds, & Chemical Equations. Hydrogen, Oxygen, & Water. What is the main difference between a mixture and a compound?. Ball-and-stick model ***check pg 87 and A-7 (appendix IIA) for colors. Space-filling molecular model.

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Empirical and Molecular Formulas

Empirical and Molecular Formulas. Empirical Formula. Empirical Formula A formula that gives the simplest whole-number ratio of the atoms of each element in a compound. CH 3 O. CH 3 O. CH 3 OOCH = C 2 H 4 O 2. CH 2 O.

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1.1.5 Types of Formula

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Chapter 8: Chemical composition

Chapter 8: Chemical composition. Chemistry 1020: Interpretive chemistry Andy Aspaas, Instructor. Atomic masses. Atomic mass unit, amu: a very small unit of mass in which masses of atoms and molecules are given A single carbon-12 atom has mass of 12 amu

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The Mole & Chemical Formulas

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III. Formula Calculations (p. 226-233)

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III. Formula Calculations (p. 226-233)

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II. Formula Calculations

The Mole. II. Formula Calculations. A. Percentage Composition. the percentage by mass of each element in a compound. 127.10 g Cu 159.17 g Cu 2 S. 32.07 g S 159.17 g Cu 2 S. A. Percentage Composition. Find the % composition of Cu 2 S. ? 100 =. %Cu =. 79.852% Cu. %S =. ? 100 =.

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DETERMINING CHEMICAL FORMULAS

DETERMINING CHEMICAL FORMULAS. What if you discovered the cure for cancer?. Any new chemical that is discovered that is a potential health care treatment must have its molecular formula submitted to the Ministry of Health.

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Calculating Empirical and Molecular Formulas

Calculating Empirical and Molecular Formulas. A chemical formula in which the ratio of the elements are in the lowest terms is called an empirical formula . For example, the empirical formula for a glucose molecule (C 6 H 12 O 6 ) is CH 2 O. All the subscripts are

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6.10 Calculating Empirical Formulas

6.10 Calculating Empirical Formulas. The empirical formula gives the lowest whole-number ratio of the atoms of the elements in a compound. It tells the kinds and relative count (atoms or moles of atoms) in molecules or formula units of a compound.

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