'Percent composition' presentation slideshows

CHAPTER 2

CHAPTER 2. CHEMICAL FORMULAS & COMPOSITION STOICHIOMETRY. Chapter Goals. Atoms and Molecules Chemical Formulas Ions and Ionic Compounds Names and Formulas of Some Ionic Compounds Atomic Weights The Mole. Chapter Goals. Formula Weights, Molecular Weights, and Moles

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I. Measuring Matter

I. Measuring Matter. Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance. .

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Unit 5

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Chapter 10

Chapter 10 . Chemical Quantities or. "Our Friend the Mole". How you measure how much?. You can measure mass, or volume, or you can count pieces. We measure mass in grams. We measure volume in liters. We count pieces in MOLES. Moles.

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Chapter 10

Chapter 10. Chemical Quantities. Chapter 10 Section 1. The Mole. Measuring matter. We measure by three different methods Counting- How many there are. Volume- How much space they take up. Mass- How much they weigh. We have to know conversion factors to relate these different measurements.

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Chapter 7: Moles and Quantities

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PERCENTAGE CALCULATIONS % = ( portion / total ) 100

PERCENTAGE CALCULATIONS % = ( portion / total ) 100. What is the percent of salt in a saltwater solution if 246.99 g of sodium chloride was added to 4.00 L of pure DI water? How much palladium is present in a 59.00 g sample of white gold (composition 90% Au & 10% Pd)?.

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Solutions

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The formula for oxalic acid is (COOH) 2 . How many atoms does each molecule contain?

The formula for oxalic acid is (COOH) 2 . How many atoms does each molecule contain?. 6 4 8 10 5. What is the molecular formula for acetic acid?. CH 3 COOH CH 3 COCH 3 CH 3 CH 2 OH CH 3 CH 2 CO 2 H CH 3 CH 2 OCH 2 CH 3. What is the formula for iron(III) oxide?. FeO 3 FeO 2 Fe 3 O 2

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Empirical Formulas

Empirical Formulas. The simplest, whole-number ratio of atoms in a molecule is called the empirical formula . Can be determined from percent composition or combining masses. The molecular formula is a multiple of the empirical formula. Empirical Formulas, Continued. Hydrogen Peroxide

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Percent Composition

Percent Composition. Chapter 10 Percent Composition and Chemical Formulas. OBJECTIVES: Describe how to calculate the percent by mass of an element in a compound. Chapter 10 - Percent Composition and Chemical Formulas. OBJECTIVES: Interpret an empirical formula.

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Sample Problems:

Sample Problems:. 1. How many grams are in 45 L of neon gas at STP?. 1 mol 22.4 L. 20.180 g 1 mol. 45 L. = 41 g. Sample Problems:. 2. How many formula units are in 36.4 g of NaCl ?. 6.02 x 10 23 form.units 1 mol. 1 mol 58.443 g. 36.4 g. = 3.75 x 10 23 formula units .

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Molar Mass & Percent Composition

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Chem Catalyst

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To understand the definition of molar mass To learn to convert between moles and mass To learn to calculate the mass p

Objectives. To understand the definition of molar mass To learn to convert between moles and mass To learn to calculate the mass percent of an element in a compound . A. Molar Mass . A compound is a collection of atoms bound together. . 1 mole of methane.

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Chapter 10 NOTES

Chapter 10 NOTES. PRACTICE PROBLEMS. Try it on your own!. A compound is formed when 9.03 g Mg combines completely with 3.48 g N. What is the percent composition of this compound? Known Mass of Mg = 9.03g Mass of N = 3.48 g Total mass of cmpd . = 12.51 g (9.03g + 3.48g) Unknown % Mg = ?

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Percent Composition

Percent Composition. Example: MgO Find molar mass of whole compound: MgO = 24.3 + 16.00 = 40.3 grams % Mg (by mass) = mass of Mg = 24.3 g x 100 = 60.3% molar mass of MgO 40.3 g

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Percent Composition

Percent Composition. Law of Definite Proportions. The Law of Definite Proportions states that a compound is always comprised of the same atoms in the same ratio, or percentage. In order to determine the percentages, we use molar mass. Percent Composition.

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http://www.sciencegeek.net/Chemistry/taters/Unit6SolutionConcentration.htm

http://www.sciencegeek.net/Chemistry/taters/Unit6SolutionConcentration.htm. Solution Concentrations. Answer the following questions. Use the formula n =cV. Check your answers by using the web site shown above. All the following questions are found on this site.

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PERCENT COMPOSITION

PERCENT COMPOSITION. The percent composition is the mass percentage of each type of atom(element) in a compound . % X = (total atomic mass of X / molar mass which contains X) For Example: Calculate the percent composition of nicotine, C 10 H 14 N 2 . Molar mass = 10C + 14H + 2N = 162 g/mol

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