CHEM1010-Fall_04-22.ppt
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This document is a chapter outline for a general chemistry course taught by Dr. Hong Zhang. It covers topics related to mole calculations, including Avogadro's number, molar mass, mole ratios in chemical equations, and using moles and mass in chemical reaction stoichiometry problems. Examples of mole and mass calculations for several chemical reactions are shown and practice problems are provided.
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2. Examples are provided for determining moles, grams, and numbers of particles from given values through step-by-step working.
3. Key stoichiometry topics covered are mole ratios, molar mass, percent composition, and solving various stoichiometric problems.
Stoichiometry
1. The concentrations given are: 1.0 E -9, 2.4 E -3, 6.7 E -7, 4.4 E -5.
2. The document discusses stoichiometry, mole conversions, molarity, and percent composition in chemistry.
3. Stoichiometry is the study of quantitative relationships in chemical reactions using molar ratios and mole conversions.
Formulas
The document discusses relative formula mass (Mr), atomic mass, empirical formula, and calculations involving chemical formulas and reactions. It provides examples of calculating Mr, percentage composition, mass of products, volume of gases produced, and determining empirical formulas from given mass ratios of elements in a compound.
Stoichiometry: Chapter 9
The document provides an introduction to stoichiometry including the four types of stoichiometry problems: (1) given and unknown amounts in moles, (2) given amount in moles and unknown in grams, (3) given amount in grams and unknown in moles, and (4) given and unknown amounts in grams. It then works through example problems of each type, calculating amounts of products or reactants using molar ratios derived from balanced chemical equations.
Ch3 stoichiometry
This document discusses stoichiometry, which is the quantitative relationships between reactants and products in chemical reactions. Some key points covered include:
- Stoichiometric amounts refer to the exact molar amounts of reactants and products in a balanced chemical equation.
- Atomic masses are given in atomic mass units (amu) which is based on carbon-12 having a mass of exactly 12 amu.
- Average atomic masses take into account the natural abundances of isotopes.
- The mole is the unit used to express amounts of substances in chemistry and 1 mole contains 6.022x1023 elementary entities.
- Molar mass is the mass in grams of 1 mole of a substance and is equal to the sum of the
Y11 stoichiometry.pptx (3).pdf
Y11
STOICHIOMETRIC
RELATIONSHIPS
REACTING MASSES AND VOLUMES
The document discusses three main topics:
1) Stoichiometric relationships can be used to calculate reacting ratios by mass and gas volume using mole ratios from chemical equations.
2) The SI and other common units used for pressure, volume, and other measurements in stoichiometry problems.
3) The key steps and concepts involved in solving various types of stoichiometry problems involving moles, masses, volumes of gases, concentrations, limiting reactants, theoretical and experimental yields.
Stoichiometry (Perhitungan Kimia/Stoikiometri)
This document provides information about stoichiometry and fundamental chemistry concepts. It discusses chemical reactions and equations, including types of reactions like combustion, decomposition, and double displacement. Five fundamental chemical laws are explained: conservation of mass, definite proportions, multiple proportions, combining volumes, and Avogadro's hypothesis. Concepts like mole, molecular mass, and formula mass are defined. Worked examples demonstrate how to use these concepts to calculate quantities in chemical reactions from mass and volume relationships.
Chemical reactions
The document discusses various chemical concepts including:
1) Empirical and molecular formulas, and how to determine them from elemental composition and molar mass data.
2) Types of chemical reactions such as decomposition, combination, double replacement, combustion, and fermentation reactions.
3) How metal oxides react with water to form alkalis/bases while non-metal oxides form acids when reacting with water.
Chemistry - Chp 12 - Stoichiometry - PowerPoint
The document discusses stoichiometry, which is the calculation of quantities in chemical reactions based on a balanced equation. It explains how to interpret balanced equations in terms of particles, moles, mass, and gas volume. It also covers how to perform stoichiometric calculations using mole-mole, mole-mass, and volume-volume conversions based on molar ratios from balanced equations.
Stoichiometry
Magnesium metal reacts with oxygen to produce magnesium oxide. Stoichiometry uses mole ratios derived from chemical equations to calculate amounts of substances involved in chemical reactions. For example, the mole ratio for the reaction 2Mg + O2 → 2MgO is 2:1:2. This can be used to determine that 4 moles of magnesium will react with oxygen to produce 4 moles of magnesium oxide. Stoichiometry problems can involve mass calculations using the formula that the number of moles equals the mass in grams divided by the molar mass in g/mol.
Chapter4
1. This document summarizes key concepts from a chapter on chemical reactions including formula weight, moles, balancing equations, stoichiometry, percent yield, and oxidation-reduction reactions.
2. Key topics covered include calculating molar mass, determining the limiting reactant and theoretical yield of a reaction, and identifying oxidation and reduction in redox reactions.
3. The chapter also discusses solubility rules, writing net ionic equations, and the heat absorbed or released by exothermic and endothermic reactions.
Chapter 3 notes
The document defines atomic mass, molar mass, molecular mass, and formula mass. It explains that atomic mass is the mass of an atom measured in atomic mass units (amu) and is based on carbon-12. Molar mass is the mass of one mole of a substance in grams. One mole contains 6.022x1023 elementary units. Molecular mass is the sum of atomic masses in a molecule. Formula mass is the sum of atomic masses in a formula unit of an ionic compound. The document provides examples of calculating molar mass, molecular mass, and formula mass from atomic masses on the periodic table.
Report in Physical Science (Stoichiometry).ppt
This document discusses various types of stoichiometry calculations including:
- Mole-mole stoichiometry conversions
- Mass-mass stoichiometry conversions
- Mole-mass stoichiometry conversions
- Sample problems are provided that demonstrate how to use the balanced chemical equations and molar relationships to solve for unknown quantities. Conversions include moles, mass, particles, volumes and relate the amounts of reactants and products in a chemical reaction.
Blb12 ch03 lecture
This document summarizes key concepts in stoichiometry including:
1) Chemical equations represent chemical reactions and show reactants on the left and products on the right. Coefficients are used to balance equations.
2) Formula weights are calculated by adding atomic weights of elements in a compound. Moles provide a connection between molecular and macroscopic scales.
3) Stoichiometric calculations use mole ratios from balanced equations to relate amounts of reactants and products. The limiting reactant determines the theoretical yield.
Chem 101 week 5
This document contains lecture notes on stoichiometry from a CHEM 101 class. It discusses concepts like writing and balancing chemical equations, determining the empirical formula of a compound from combustion analysis data, calculating amounts of reactants and products using mole ratios from balanced equations, identifying the limiting reactant, and calculating theoretical and percent yields. Key steps in stoichiometry problems are outlined, such as converting masses to moles and using mole ratios to determine unknown quantities. Examples are provided to demonstrate these concepts.
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- 1. Department of Chemistry CHEM1010 General Chemistry *********************************************** Instructor: Dr. Hong Zhang Foster Hall, Room 221 Tel: 931-6325 Email: hzhang@tntech.edu