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Stoichiometry

Chapter 5b

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Chemistry 1210: Introduction to General Chemistry Dr. Gina M. Florio 27 Sept. 2012 Jespersen, Brady, Hyslop Chapter 5B Molecular View of Reactions in Aqueous Solution Properties of Solutions: Quantitative Composition The molar concentration or molarity (M) is defined as: units of M = mol/L (mol L-1) Example: How many grams of AgNO3 are needed to prepare 250 mL of a 0.0125 M AgNO3 solution? NOTE: You can also solve this for concentration OR liters of solution CH. 5 Properties of Solutions: Quantitative Composition Solutions of high concentration can be diluted to make solutions of lower concentration. Dilution: CH. 5 Example: How much 1.0 M CuSO4 (aq) solution is required to prepare 250 mL of a 0.10 M CuSO4 (aq) solution? How much water is required? Solution Stoichiometry CH. 5

Chapter 4

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Chemistry 1210: General Chemistry Dr. Gina M. Florio 13 September 2012 Jespersen, Brady, Hyslop, Chapter 4 The Mole and Stoichiometry CHE 1210 Lecture Slides G.M. Florio 1 Conversion Factors Conversion Factor ? relates one quantity to another ? used to convert between two units in chemistry What is my height in centimeters (cm) if I am 5 feet 4 inches tall? 1. How many inches are in a foot? 2. How many inches are in a centimeter? 12 inches = 1 foot 1 inch = 2.54 cm Factor Label Method The factor-label method, or dimensional analysis lets us treat a numerical problem as one involving a conversion from one kind of units to another using conversion factors.

Bob Jones PPT Notes -- Chapter 10c

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Physical quantities

Physical chemistry

Introductory physics

Amount of substance

Gases and the Mole Gay-Lussac formulated the law of combining volumes. Law of Combining Volumes Gases at the same temperature and pressure react with one another in volume ratios of small whole numbers. Law of Combining Volumes Example 1: H2 + Cl2 2HCl 1 L + 1 L 2 L Law of Combining Volumes Example 2: 2H2 + O2 2H2O 2 L + 1 L 2 L Avogadro?s law The volume of a gas, maintained at a constant temperature and pressure, is directly proportional to the number of moles of the gas. Molar Volume the volume that a mole of gas occupies at standard temperature and pressure Molar Volume 1 mole of ANY gas at STP occupies 22.4 L. Sample Problem 1 What volume would 7 moles of carbon dioxide occupy at STP? = 157 L CO2 7 mol CO2 22.4 L 1 mol Change 228 L of O2 at STP to moles. 470 moles 426 moles

Bob Jones PPT Notes -- Chapter 9b

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Chemical reactions

Limiting reagent

Stoichiometry 1 Literally means ?to measure the elements? Answers questions like?How much is needed?? and ?How much is produced?? Stoichiometry Unit analysis 365 days 1 year 24 hrs 1 day 3600 sec. 1 hr 1 year How many seconds are in a year? = 31,536,000 sec. Unit analysis We use unit analysis in stoichiometric problems also. Grams-to-moles conversion factors are found in the periodic table. Unit analysis Mole-to-mole conversion factors are found in the coefficients of the equation. A mole-to-mole conversion changes moles of one substance to moles of another substance. ?Skeleton Equation?

Bob Jones PPT Notes -- Chapter 8c

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Chemical engineering

Chemical equation

Chemical reactions

Chemical kinetics

Element-reactant-product table

Thermochemical equation

Writing Equations Chemical Equations Math equations show equalities. Chemical equations show processes (one chemical changes to another chemical). A Chemical Equation Must: Identify all the substances involved. Show the composition of the substances (use formulas). A Chemical Equation Must: Account for all the atoms. (There must be the same number of atoms of every element on both sides of the equation.) Parts of an Equation Reactants Products Coefficients Arrow Example reactants Ca(HCO3)2 + Ca(OH)2 2 H2O + 2 CaCO3 products The ?2? is a coefficient to tell how many molecules of each compound are present. What tells you how many atoms of an element are in a molecule? Symbol Subscript Coefficient Catalyst Question 7 Special Symbols in Equations g?: A gas was produced.

Chapter 3/4

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Physical chemistry

Equilibrium chemistry

Chemical reactions

Strong electrolyte

Chemical equation

Limiting reagent

Claire Rafson Chapter 3 notes 3.1 You can count things by weight 3.2 Atomic mass determined on a mass spectrometer Average atomic mass = atomic mass for the element 3.3 Avogadro?s number = 6.02214 X 10^23 1 mole = avogadro?s number 3.4 molar mass= mass in grams of one mole of the compound 3.5 Percent comp of compounds Mass percent- weight percent can be computed by comparing the mass of carbon Find moles of all divide by smallest number find whole number etc. 3.6 Molecular formula= (empirical formula)n N is an integer To find molec formula take molar mass/ empirical formula mass and that is n SEE PAGE 96 IF CONFUSED 3.7- Chemical Reactions- Reactants on left and products on the right. Aq- dissolved in water 3.8- Balance reactions 3.9- Stoichiometry-

Chapter 2

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Chemical properties

Amount of substance

Chemical element

Chapter 2.1- 2.3 (pages 41-48) Law of conservation of mass- Mass is neither created nor destroyed Law of definite proportion- a given compound always contains exactly the same proportion of elements by mass. Law of multiple proportions- When two elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to small whole numbers Dalton?s Atomic Theory- -Each element is made up of atoms -The atoms of a given element are identical -Chemical compounds are formed when atoms of diff elements combine with each other -Chemical reactions involve reorganization of the atoms Dalton prepared first table of atomic masses

chem

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Chemical engineering

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Chemical bonding

Quantum chemistry

Chemical reaction

Chemical element

CALIFORNIA STANDARDS TEST CHEMISTRY (Blueprint adopted by the State Board of Education 10/2002) CALIFORNIA CONTENT STANDARDS: CHEMISTRY # of Items % Atomic and Molecular Structure 6 10.0% 1. The periodic table displays the elements in increasing atomic number and shows how periodicity of the physical and chemical properties of the elements relates to atomic structure. As a basis for understanding this concept: a. Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass. 1 b. Students know how to use the periodic table to identify metals, semimetals, non-metals, and halogens. 1

chem

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Chemical engineering

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CALIFORNIA STANDARDS TEST CHEMISTRY (Blueprint adopted by the State Board of Education 10/2002) CALIFORNIA CONTENT STANDARDS: CHEMISTRY # of Items % Atomic and Molecular Structure 6 10.0% 1. The periodic table displays the elements in increasing atomic number and shows how periodicity of the physical and chemical properties of the elements relates to atomic structure. As a basis for understanding this concept: a. Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass. 1 b. Students know how to use the periodic table to identify metals, semimetals, non-metals, and halogens. 1

chem

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Chemical engineering

Chemical properties

Chemical bonding

Quantum chemistry

Chemical reaction

Chemical element

CALIFORNIA STANDARDS TEST CHEMISTRY (Blueprint adopted by the State Board of Education 10/2002) CALIFORNIA CONTENT STANDARDS: CHEMISTRY # of Items % Atomic and Molecular Structure 6 10.0% 1. The periodic table displays the elements in increasing atomic number and shows how periodicity of the physical and chemical properties of the elements relates to atomic structure. As a basis for understanding this concept: a. Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass. 1 b. Students know how to use the periodic table to identify metals, semimetals, non-metals, and halogens. 1

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