HOW TO SOLVE CALCULATIONS IN SCIENCE..pptxTEMPLEEKE
Carrying out calculations is an inevitable activity in solving problems in Science. This masterpiece highlights the causes of incompetence in handling calculations in Science. Four stages of handling calculations are explained and Ten guidelines for handling calculations are presented. This is a must-read for every student and instructor of Science.
The document summarizes key concepts in thermodynamics and heat transfer. It defines important terms like temperature, heat, work, and entropy. It also outlines the first and second laws of thermodynamics. The first law states that energy is conserved in thermal processes, such that the change in internal energy of a system equals heat added minus work done. The second law states that the entropy of the universe increases over time as energy spreads out. The document provides important equations related to heat, work, and efficiency and lists common units used in thermodynamics.
When objects are heated, they expand due to thermal expansion. Thermal expansion occurs because the energy stored in the intermolecular bonds between atoms increases with temperature, causing the molecular bonds to lengthen. Examples of applications of thermal expansion include metal framed windows using rubber spacers, metal hot water pipes avoiding long straight lengths, and large structures like bridges employing expansion joints. Thermometers also demonstrate thermal expansion through the constrained flow of liquid in a tube due to changes in volume from temperature variations.
This document discusses various concepts relating to aqueous reactions and solution chemistry. It defines key terms including solutions, electrolytes, dissociation, strong and weak electrolytes, and precipitation reactions. It also covers types of reactions such as acid-base, gas-forming, oxidation-reduction, displacement and metathesis reactions. Additionally, it discusses concepts like oxidation numbers, molarity and titrations which are important for understanding reaction stoichiometry in aqueous solutions.
The electronegativity of an element is a measure of how strongly it attracts electrons in a covalent bond. Electronegativity increases left to right and top to bottom in a period, and metals have the lowest values while nonmetals have the highest. The difference in electronegativity between two bonded atoms indicates bond type - ionic bonds form when difference is >1.7, covalent bonds form when difference is <1.7, and polar covalent bonds form for differences in between. Electronegativity values can be used to predict and investigate bond types.
Thermochemistry is the study of heat changes in chemical reactions and phase changes. There are two types of energy - kinetic energy, which is the energy of motion, and potential energy, which is stored energy like that in chemical bonds. Energy cannot be created or destroyed, only converted between kinetic and potential forms. Heat is a transfer of energy between objects due to a temperature difference, flowing from warmer to cooler until equal temperatures are reached. Exothermic reactions release heat while endothermic reactions absorb heat from their surroundings.
The document discusses the Bohr model of the atom, including that the number of electrons in an atom equals its atomic number, electrons fill energy levels from the outside in, and the first energy level can contain 2 electrons while the second and third can contain 8 each. It prompts the reader to draw Bohr diagrams for lithium, oxygen, and chlorine atoms.
HOW TO SOLVE CALCULATIONS IN SCIENCE..pptxTEMPLEEKE
Carrying out calculations is an inevitable activity in solving problems in Science. This masterpiece highlights the causes of incompetence in handling calculations in Science. Four stages of handling calculations are explained and Ten guidelines for handling calculations are presented. This is a must-read for every student and instructor of Science.
The document summarizes key concepts in thermodynamics and heat transfer. It defines important terms like temperature, heat, work, and entropy. It also outlines the first and second laws of thermodynamics. The first law states that energy is conserved in thermal processes, such that the change in internal energy of a system equals heat added minus work done. The second law states that the entropy of the universe increases over time as energy spreads out. The document provides important equations related to heat, work, and efficiency and lists common units used in thermodynamics.
When objects are heated, they expand due to thermal expansion. Thermal expansion occurs because the energy stored in the intermolecular bonds between atoms increases with temperature, causing the molecular bonds to lengthen. Examples of applications of thermal expansion include metal framed windows using rubber spacers, metal hot water pipes avoiding long straight lengths, and large structures like bridges employing expansion joints. Thermometers also demonstrate thermal expansion through the constrained flow of liquid in a tube due to changes in volume from temperature variations.
This document discusses various concepts relating to aqueous reactions and solution chemistry. It defines key terms including solutions, electrolytes, dissociation, strong and weak electrolytes, and precipitation reactions. It also covers types of reactions such as acid-base, gas-forming, oxidation-reduction, displacement and metathesis reactions. Additionally, it discusses concepts like oxidation numbers, molarity and titrations which are important for understanding reaction stoichiometry in aqueous solutions.
The electronegativity of an element is a measure of how strongly it attracts electrons in a covalent bond. Electronegativity increases left to right and top to bottom in a period, and metals have the lowest values while nonmetals have the highest. The difference in electronegativity between two bonded atoms indicates bond type - ionic bonds form when difference is >1.7, covalent bonds form when difference is <1.7, and polar covalent bonds form for differences in between. Electronegativity values can be used to predict and investigate bond types.
Thermochemistry is the study of heat changes in chemical reactions and phase changes. There are two types of energy - kinetic energy, which is the energy of motion, and potential energy, which is stored energy like that in chemical bonds. Energy cannot be created or destroyed, only converted between kinetic and potential forms. Heat is a transfer of energy between objects due to a temperature difference, flowing from warmer to cooler until equal temperatures are reached. Exothermic reactions release heat while endothermic reactions absorb heat from their surroundings.
The document discusses the Bohr model of the atom, including that the number of electrons in an atom equals its atomic number, electrons fill energy levels from the outside in, and the first energy level can contain 2 electrons while the second and third can contain 8 each. It prompts the reader to draw Bohr diagrams for lithium, oxygen, and chlorine atoms.
Atoms are the building blocks of matter and consist of a nucleus surrounded by electrons. The nucleus contains protons and neutrons, and most of an atom's mass is in the nucleus. Electrons orbit the nucleus in energy levels. The number of protons determines the element and is an atom's atomic number. An atom's atomic mass comes from the total number of protons and neutrons.
This document provides a summary of key chemistry concepts related to liquids and solids. It defines intermolecular forces like London dispersion forces, dipole-dipole forces, and hydrogen bonding. It also explains properties of solids like crystalline and amorphous structure. Phase changes between solid, liquid, and gas are discussed, including the energies involved in melting, vaporization, and sublimation. Vapor pressure equilibrium is defined as the state where the rate of evaporation equals the rate of condensation.
The imperial measurement system originated from human body parts and varied over time. A cubit was the length from the elbow to the tip of the fingers. An inch was three grains of barley laid end to end. A pound was the weight of a bag of 7,200 grains of barley. Imperial units like feet, yards, miles, ounces, pounds and more were defined, but conversions between units grew increasingly complex over centuries of use.
This document provides a summary of key concepts for electron configuration in high school chemistry, including:
1) Electrons fill subshells according to the aufbau principle to achieve lowest energy, with Hund's rule specifying that electrons occupy each orbital singly before pairing up.
2) The four subshells are s, p, d, and f, with set numbers of orbitals and maximum electrons in each. Valence electrons are in the outermost shell.
3) Electron configuration can be written using boxes and arrows, spectroscopic notation, or noble gas notation, with examples provided.
This document provides a summary of key concepts for predicting products in chemical reactions on the AP Chemistry exam. It defines common reaction types like precipitation and acid-base reactions. It outlines the steps to take to determine the molecular, complete ionic, and net ionic equations for different reaction types. These include double replacement, acid-base, decomposition, combustion, redox, and complex ion formation reactions. Solubility rules are also summarized to predict if a compound will precipitate out of solution. The document concludes with guidance on how to convert word problems into balanced chemical equations.
Rate of reaction is defined as the change in quantity of reactants or products per unit time. The average rate is calculated over an interval of time, while the instantaneous rate is the actual rate at a given time. Several factors affect the rate of reaction, including the total surface area and concentration of reactants, temperature, use of catalysts, and pressure for gaseous reactants. According to collision theory, the rate of reaction depends on the frequency and effectiveness of collisions between reactant particles, which must achieve the minimum activation energy and correct orientation.
The document discusses the topic of catalysis. Some key points:
- Berzelius coined the term "catalysis" in 1836 to describe reactions that are accelerated by substances that remain unchanged after the reaction.
- Catalysts work by providing an alternative reaction pathway which has a lower activation energy, allowing a greater proportion of particles to react.
- There are two main types of catalysis: heterogeneous catalysis where the catalyst is in a different phase than the reactants, and homogeneous catalysis where the catalyst and reactants are in the same phase.
- Many important industrial processes rely on catalysis such as the Haber process, contact process, and catalytic converters. Catalysis plays a key role
This document provides an overview of key concepts in stoichiometry, including:
- Stoichiometry uses mole ratios in balanced chemical equations to relate amounts of reactants and products. Dimensional analysis converts between units using molar mass, concentration, molar volume, and other relationships.
- The limiting reactant is the first reactant to be used up in a chemical reaction. It determines the maximum amount of product that can be formed.
- Percent yield compares the actual yield from a chemical reaction to the theoretical yield calculated from stoichiometry.
- KUDUS is a mnemonic for solving stoichiometry word problems: identify what is Known, Unknown, the Definitions needed, perform the Output calculation, and
This document discusses a lecture on electrochemistry. It covers key concepts like electrolysis, Faraday's laws of electrolysis, and electrochemical cells.
Some key points covered include that electrolysis is the decomposition of a compound by an electric current, and involves oxidation and reduction reactions. Faraday's first law states the mass of a substance produced by electrolysis is directly proportional to the quantity of electricity used. Faraday's second law relates the masses of different substances deposited to their equivalent masses. An electrochemical cell uses a redox reaction to produce an electrical current.
5.4 exothermic and endothermic reactionsMartin Brown
This document discusses exothermic and endothermic reactions. Exothermic reactions release heat, while endothermic reactions absorb heat. Combustion reactions of hydrocarbons like methane and propane are exothermic, producing carbon dioxide, water vapor, and large amounts of heat. The heat of reaction, ΔH, indicates whether a reaction is exothermic (negative ΔH) or endothermic (positive ΔH). Bond energies represent the energy required to break bonds, while heat of combustion measures the heat released from complete combustion. A bomb calorimeter is used to accurately measure heats of combustion by igniting samples in excess oxygen. Hess's law states that the heat change of a reaction depends only on
The document discusses kinetics and reaction rates. It defines kinetics as the branch of chemistry that studies the speed or rate of chemical reactions. It explains that reaction rates can be measured by changes in concentration, temperature, or pressure over time. The rate depends on factors like the nature of reactants, concentration, temperature, catalysts, surface area, and pressure. Reactions may occur in multiple steps through reaction intermediates rather than a single step. The collision theory and concept of activation energy are introduced to explain why certain collisions result in reactions. Reaction coordinate diagrams are used to illustrate the energy changes in reactions.
Thermal diffusion, also known as the Soret effect, is the separation of components in a mixture due to a temperature gradient. When a temperature gradient is applied to a mixture, the components diffuse at different rates depending on their mass and interactions. Lighter components typically move toward the hot surface while heavier components move toward the cold surface. Thermal diffusion can be used to separate isotopes using static cells or thermogravitational columns, where natural convection enhances the separation. The efficiency depends on factors like temperature difference, particle size, thermal conductivity, and column dimensions. Applications include isotope separation and analytical separations.
IB Chemistry on Periodic Trends, Effective Nuclear Charge and Physical proper...Lawrence kok
This document provides a tutorial on periodic trends in physical and chemical properties for elements in periods 2 and 3 of the periodic table. It discusses how ionization energy generally increases across a period as the nuclear charge increases, but may decrease between certain elements due to electrons entering new orbitals farther from the nucleus or due to increased electron-electron repulsion with multiple electrons in the same orbital. Specifically, it notes the ionization energy decreases from beryllium to boron and from nitrogen to oxygen in period 2, and from magnesium to aluminum and from phosphorus to sulfur in period 3 for these reasons.
Includes a discussion of Voltaic and electrolytic cells, the Nernst equation and the relationship between electrochemical processes, chemical equilibrium and free energy.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
The document discusses factors that affect the rate of chemical reactions, including:
1) Temperature, concentration, pressure, particle size, and presence of catalysts can increase the rate of reaction by increasing the probability of effective collisions between reacting particles.
2) The rate of reaction generally increases with increasing temperature, concentration, and pressure or decreasing particle size because these factors increase the likelihood of collisions possessing sufficient energy to produce products.
3) Catalysts increase the rate of reaction by lowering the activation energy of the reactants through alternative reaction pathways.
Chemical reactions require energy to break and form bonds. Exothermic reactions release more energy than they absorb, causing an increase in temperature. Endothermic reactions absorb more energy than they release, causing a decrease in temperature. All reactions require a minimum amount of activation energy to start. The rate of reaction depends on factors like concentration, temperature, surface area, catalysts and inhibitors. Catalysts lower the activation energy and speed up reactions without being used up.
The document discusses chemical bonding, including:
1. Defining ionic and covalent bonding, and explaining how different types of bonds are formed through electron sharing or transfer.
2. Describing the properties of ionic and covalent compounds, such as high melting points for ionic solids and variable states of matter for covalent substances.
3. Illustrating examples of single, double, and triple covalent bonds through Lewis dot structures of molecules like H2, O2, and N2.
Lewis structuresvsepr theory cheat sheetTimothy Welsh
1. The document provides an overview of key concepts for Lewis structures and VSEPR theory, including how to draw Lewis structures for covalent compounds and ions.
2. It explains valence shell electron pair repulsion theory (VSEPR) which is used to predict the 3D shape of molecules based on electron pairs around a central atom.
3. A table is included that lists common molecular geometries determined by VSEPR theory based on the number of electron regions around the central atom.
This document provides an overview of key concepts and equations related to gases in chemistry. It defines gas laws and the kinetic molecular theory, including assumptions like molecules having negligible volume. Common gas laws are described, such as Boyle's, Charles', Dalton's and the combined gas law. Equations are provided for ideal and real gases. The document also covers gas stoichiometry, effusion, diffusion, and Graham's laws relating molecular mass to rates of effusion and diffusion. Strategies are suggested for attacking gas law problems by identifying quantities, writing knowns and unknowns symbolically, choosing the appropriate equation, and solving.
This document provides an overview of the key concepts covered in 5 sections of a chapter on energy and chemical change:
Section 15.1 defines energy and distinguishes between potential and kinetic energy. It relates chemical potential energy to heat released or absorbed in chemical reactions.
Section 15.2 describes how calorimetry is used to measure energy changes and defines enthalpy and enthalpy changes.
Section 15.3 explains how to write thermochemical equations and describes energy changes during state changes.
Section 15.4 discusses calculating enthalpy changes using Hess's law and standard enthalpies of formation.
Section 15.5 differentiates between spontaneous and nonspontaneous processes and explains how entropy
Atoms are the building blocks of matter and consist of a nucleus surrounded by electrons. The nucleus contains protons and neutrons, and most of an atom's mass is in the nucleus. Electrons orbit the nucleus in energy levels. The number of protons determines the element and is an atom's atomic number. An atom's atomic mass comes from the total number of protons and neutrons.
This document provides a summary of key chemistry concepts related to liquids and solids. It defines intermolecular forces like London dispersion forces, dipole-dipole forces, and hydrogen bonding. It also explains properties of solids like crystalline and amorphous structure. Phase changes between solid, liquid, and gas are discussed, including the energies involved in melting, vaporization, and sublimation. Vapor pressure equilibrium is defined as the state where the rate of evaporation equals the rate of condensation.
The imperial measurement system originated from human body parts and varied over time. A cubit was the length from the elbow to the tip of the fingers. An inch was three grains of barley laid end to end. A pound was the weight of a bag of 7,200 grains of barley. Imperial units like feet, yards, miles, ounces, pounds and more were defined, but conversions between units grew increasingly complex over centuries of use.
This document provides a summary of key concepts for electron configuration in high school chemistry, including:
1) Electrons fill subshells according to the aufbau principle to achieve lowest energy, with Hund's rule specifying that electrons occupy each orbital singly before pairing up.
2) The four subshells are s, p, d, and f, with set numbers of orbitals and maximum electrons in each. Valence electrons are in the outermost shell.
3) Electron configuration can be written using boxes and arrows, spectroscopic notation, or noble gas notation, with examples provided.
This document provides a summary of key concepts for predicting products in chemical reactions on the AP Chemistry exam. It defines common reaction types like precipitation and acid-base reactions. It outlines the steps to take to determine the molecular, complete ionic, and net ionic equations for different reaction types. These include double replacement, acid-base, decomposition, combustion, redox, and complex ion formation reactions. Solubility rules are also summarized to predict if a compound will precipitate out of solution. The document concludes with guidance on how to convert word problems into balanced chemical equations.
Rate of reaction is defined as the change in quantity of reactants or products per unit time. The average rate is calculated over an interval of time, while the instantaneous rate is the actual rate at a given time. Several factors affect the rate of reaction, including the total surface area and concentration of reactants, temperature, use of catalysts, and pressure for gaseous reactants. According to collision theory, the rate of reaction depends on the frequency and effectiveness of collisions between reactant particles, which must achieve the minimum activation energy and correct orientation.
The document discusses the topic of catalysis. Some key points:
- Berzelius coined the term "catalysis" in 1836 to describe reactions that are accelerated by substances that remain unchanged after the reaction.
- Catalysts work by providing an alternative reaction pathway which has a lower activation energy, allowing a greater proportion of particles to react.
- There are two main types of catalysis: heterogeneous catalysis where the catalyst is in a different phase than the reactants, and homogeneous catalysis where the catalyst and reactants are in the same phase.
- Many important industrial processes rely on catalysis such as the Haber process, contact process, and catalytic converters. Catalysis plays a key role
This document provides an overview of key concepts in stoichiometry, including:
- Stoichiometry uses mole ratios in balanced chemical equations to relate amounts of reactants and products. Dimensional analysis converts between units using molar mass, concentration, molar volume, and other relationships.
- The limiting reactant is the first reactant to be used up in a chemical reaction. It determines the maximum amount of product that can be formed.
- Percent yield compares the actual yield from a chemical reaction to the theoretical yield calculated from stoichiometry.
- KUDUS is a mnemonic for solving stoichiometry word problems: identify what is Known, Unknown, the Definitions needed, perform the Output calculation, and
This document discusses a lecture on electrochemistry. It covers key concepts like electrolysis, Faraday's laws of electrolysis, and electrochemical cells.
Some key points covered include that electrolysis is the decomposition of a compound by an electric current, and involves oxidation and reduction reactions. Faraday's first law states the mass of a substance produced by electrolysis is directly proportional to the quantity of electricity used. Faraday's second law relates the masses of different substances deposited to their equivalent masses. An electrochemical cell uses a redox reaction to produce an electrical current.
5.4 exothermic and endothermic reactionsMartin Brown
This document discusses exothermic and endothermic reactions. Exothermic reactions release heat, while endothermic reactions absorb heat. Combustion reactions of hydrocarbons like methane and propane are exothermic, producing carbon dioxide, water vapor, and large amounts of heat. The heat of reaction, ΔH, indicates whether a reaction is exothermic (negative ΔH) or endothermic (positive ΔH). Bond energies represent the energy required to break bonds, while heat of combustion measures the heat released from complete combustion. A bomb calorimeter is used to accurately measure heats of combustion by igniting samples in excess oxygen. Hess's law states that the heat change of a reaction depends only on
The document discusses kinetics and reaction rates. It defines kinetics as the branch of chemistry that studies the speed or rate of chemical reactions. It explains that reaction rates can be measured by changes in concentration, temperature, or pressure over time. The rate depends on factors like the nature of reactants, concentration, temperature, catalysts, surface area, and pressure. Reactions may occur in multiple steps through reaction intermediates rather than a single step. The collision theory and concept of activation energy are introduced to explain why certain collisions result in reactions. Reaction coordinate diagrams are used to illustrate the energy changes in reactions.
Thermal diffusion, also known as the Soret effect, is the separation of components in a mixture due to a temperature gradient. When a temperature gradient is applied to a mixture, the components diffuse at different rates depending on their mass and interactions. Lighter components typically move toward the hot surface while heavier components move toward the cold surface. Thermal diffusion can be used to separate isotopes using static cells or thermogravitational columns, where natural convection enhances the separation. The efficiency depends on factors like temperature difference, particle size, thermal conductivity, and column dimensions. Applications include isotope separation and analytical separations.
IB Chemistry on Periodic Trends, Effective Nuclear Charge and Physical proper...Lawrence kok
This document provides a tutorial on periodic trends in physical and chemical properties for elements in periods 2 and 3 of the periodic table. It discusses how ionization energy generally increases across a period as the nuclear charge increases, but may decrease between certain elements due to electrons entering new orbitals farther from the nucleus or due to increased electron-electron repulsion with multiple electrons in the same orbital. Specifically, it notes the ionization energy decreases from beryllium to boron and from nitrogen to oxygen in period 2, and from magnesium to aluminum and from phosphorus to sulfur in period 3 for these reasons.
Includes a discussion of Voltaic and electrolytic cells, the Nernst equation and the relationship between electrochemical processes, chemical equilibrium and free energy.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
The document discusses factors that affect the rate of chemical reactions, including:
1) Temperature, concentration, pressure, particle size, and presence of catalysts can increase the rate of reaction by increasing the probability of effective collisions between reacting particles.
2) The rate of reaction generally increases with increasing temperature, concentration, and pressure or decreasing particle size because these factors increase the likelihood of collisions possessing sufficient energy to produce products.
3) Catalysts increase the rate of reaction by lowering the activation energy of the reactants through alternative reaction pathways.
Chemical reactions require energy to break and form bonds. Exothermic reactions release more energy than they absorb, causing an increase in temperature. Endothermic reactions absorb more energy than they release, causing a decrease in temperature. All reactions require a minimum amount of activation energy to start. The rate of reaction depends on factors like concentration, temperature, surface area, catalysts and inhibitors. Catalysts lower the activation energy and speed up reactions without being used up.
The document discusses chemical bonding, including:
1. Defining ionic and covalent bonding, and explaining how different types of bonds are formed through electron sharing or transfer.
2. Describing the properties of ionic and covalent compounds, such as high melting points for ionic solids and variable states of matter for covalent substances.
3. Illustrating examples of single, double, and triple covalent bonds through Lewis dot structures of molecules like H2, O2, and N2.
Lewis structuresvsepr theory cheat sheetTimothy Welsh
1. The document provides an overview of key concepts for Lewis structures and VSEPR theory, including how to draw Lewis structures for covalent compounds and ions.
2. It explains valence shell electron pair repulsion theory (VSEPR) which is used to predict the 3D shape of molecules based on electron pairs around a central atom.
3. A table is included that lists common molecular geometries determined by VSEPR theory based on the number of electron regions around the central atom.
This document provides an overview of key concepts and equations related to gases in chemistry. It defines gas laws and the kinetic molecular theory, including assumptions like molecules having negligible volume. Common gas laws are described, such as Boyle's, Charles', Dalton's and the combined gas law. Equations are provided for ideal and real gases. The document also covers gas stoichiometry, effusion, diffusion, and Graham's laws relating molecular mass to rates of effusion and diffusion. Strategies are suggested for attacking gas law problems by identifying quantities, writing knowns and unknowns symbolically, choosing the appropriate equation, and solving.
This document provides an overview of the key concepts covered in 5 sections of a chapter on energy and chemical change:
Section 15.1 defines energy and distinguishes between potential and kinetic energy. It relates chemical potential energy to heat released or absorbed in chemical reactions.
Section 15.2 describes how calorimetry is used to measure energy changes and defines enthalpy and enthalpy changes.
Section 15.3 explains how to write thermochemical equations and describes energy changes during state changes.
Section 15.4 discusses calculating enthalpy changes using Hess's law and standard enthalpies of formation.
Section 15.5 differentiates between spontaneous and nonspontaneous processes and explains how entropy
This document provides information about two types of covalent substances: simple molecular substances and giant covalent structures. Simple molecular substances have weak intermolecular forces between molecules, resulting in low melting and boiling points. By contrast, giant covalent structures have very strong covalent bonds between atoms, giving them very high melting and boiling points. Examples of giant covalent structures include diamond, silicon dioxide, and graphite. The document also asks questions about the properties and comparisons of these different covalent substances.
The document discusses the mole concept in chemistry. It provides guide cards explaining what a mole is, how to calculate molar mass, and how to convert between moles, mass, and number of particles. It includes activity cards with practice problems on these topics. The goal is to help students understand intricate topics in chemistry, like the mole, and enhance their critical thinking skills.
Chapter 1 fundamentals of biochemical engineeringErmias Sheberu
Here is a stoichiometric equation summarizing the metabolic pathway of glycolysis from glucose to pyruvate:
C6H12O6 → 2C3H4O3 + 2ATP + 2NADH + 2H+
This equation shows that during glycolysis, 1 molecule of glucose is broken down into 2 molecules of pyruvate with the production of 2 ATP molecules, 2 NADH molecules, and 2 hydrogen ions.
Q2. Write balanced chemical equation for fermentation of pyruvate to ethanol and CO2
The document discusses the mole concept and how to calculate molecular and formula mass. It defines formula mass as the sum of the atomic weights in an empirical formula, and molecular mass as the sum from the molecular formula. It provides steps to calculate molecular mass by determining atoms, finding atomic masses from the periodic table, and summing the products. The document also defines a mole as a quantity containing 6.02x1023 particles, the number of atoms in 12g of carbon-12. It can be used to convert between mass and number of moles.
The document discusses stoichiometry and mole ratios. It defines stoichiometry as calculating substances in a chemical reaction. The objectives are to define stoichiometry and determine mole ratios from a balanced equation. Key questions are defining stoichiometry, mole ratios, and how ratios are determined from a balanced equation. The document also defines the mole as the amount of substance with the same number of particles as 12 grams of carbon-12 and discusses using moles, atoms, ions, and molecules to count particles in chemical entities.
This document provides an introduction to biochemical macromolecules by defining key terms like polymer, monomer, and the "Big 4" macromolecules. It discusses that polymers are long chains made of repeating monomer units, and the Big 4 include proteins, carbohydrates, and nucleic acids. Examples are given of analogies to explain polymers and monomers, like a train being made of connected cars. Food labels contain carbohydrates, proteins, and fats. The 4th macromolecule is nucleic acids like DNA and RNA.
The document provides instructions for calculating the empirical formula from percent composition data. It explains that the empirical formula represents the simplest whole number ratio of elements in a compound. The steps outlined are: 1) Convert the percentage of each element to grams. 2) Calculate the moles of each element using molar mass conversion factors. 3) Divide each mole value by the smallest mole value to determine the simplest mole ratio. 4) Multiply the ratios by the smallest number if needed to obtain whole numbers. An example problem is provided to demonstrate calculating the empirical formula of methyl acetate from its given percent composition.
This document provides an overview and description of an Analytical Chemistry course. It discusses the course objectives, which include developing fundamental theoretical and practical skills in analytical chemistry. It also outlines the course contents, which cover topics like data handling, stoichiometric calculations, acid-base equilibria, and oxidation-reduction reactions. The document discusses the teaching approach, which involves lectures and discussions. It lists the primary and additional references for the course.
The document provides notes on moles, molar mass, empirical formulas, and molecular formulas, including how to convert between units like grams, moles, particles, and volume using molar mass and stoichiometry. It defines key terms like moles, molar mass, empirical formula, and molecular formula. Examples are provided for calculating molar mass, moles, empirical formulas, and molecular formulas.
1. The document provides an overview of basic concepts in chemistry covered in an 11th grade chemistry course, including the divisions of chemistry, laws of chemical combination, Dalton's atomic theory, significant figures, stoichiometric coefficients, the mole, Avogadro's number, and the limiting reagent.
2. Key concepts are explained, such as how the limiting reagent determines how much of a product can be formed in a chemical reaction.
3. Example problems are provided to illustrate calculating molarity, empirical and molecular formulas, and amount of products formed using stoichiometric calculations and identifying the limiting reagent.
Stoichiometry is the study of quantitative relationships between reactants and products in chemical reactions based on mole ratios from balanced equations. Key concepts include:
1) Balanced equations show mole, mass, and particle relationships between reactants and products
2) Limiting reactants determine the maximum amount of product that can be formed
3) Excess reactants remain after the limiting reactant is used up in the reaction
- Calculate the mass of NaOH needed:
Molar mass of NaOH = 40 g/mol
Moles of NaOH needed = Concentration x Volume = 0.1 mol/L x 0.25 L = 0.025 mol
Mass of NaOH needed = Moles x Molar mass = 0.025 mol x 40 g/mol = 1 g
- Weigh out 1 g of NaOH and transfer to a 250 mL volumetric flask.
- Add about 150 mL of distilled water to dissolve the NaOH.
- Dilute to the mark with distilled water and invert to mix. The solution is now 0.1 M NaOH.
B. Preparing solutions by dilution
This document provides an introduction to chemistry, including:
- Defining chemistry as the study of matter, its structure and properties, and how matter changes.
- Explaining that chemistry is involved in many everyday materials and has various career applications.
- Describing the basic units that make up all matter - atoms, elements, and compounds.
- Discussing properties of matter like physical and chemical properties, and physical and chemical changes.
- Introducing important concepts like the periodic table, the scientific method, and laboratory safety procedures and equipment.
This document provides an overview of chemistry including:
- Chemistry is the study of matter, its structure and properties, and how matter changes.
- There are many careers in fields like engineering, medicine, and more that involve chemistry.
- Matter is made up of elements, compounds, and mixtures. Properties include physical properties that can be observed without changing identity, and chemical properties involving changes to form new substances.
This presentation discusses methods for determining the number average molecular weight (Mn) of polymers. It describes techniques such as cryoscopy (freezing point depression), ebullioscopy (boiling point elevation), and osmometry including vapor phase osmometry and membrane osmometry. It also discusses end group analysis and how it can be used to calculate Mn by determining the functionality of end groups. The techniques vary in the molecular weight ranges they are applicable to, with cryoscopy and ebullioscopy typically able to measure up to Mn of 30,000 and osmometry and end group analysis having broader ranges.
This document discusses stoichiometry and concepts related to counting atoms and molecules. It introduces atomic masses and how mass spectrometry can be used to determine relative atomic masses. The mole is defined as 6.022x1023 atoms, which allows chemists to convert between the number of atoms or molecules and mass. Empirical and molecular formulas are distinguished, and methods for determining formulas from elemental composition data are presented. Chemical equations are introduced as a way to represent chemical reactions by balancing reactants and products.
This document provides instructions and examples for calculating molar mass, determining the number of moles, calculating percent composition to determine an empirical formula, and using the empirical formula to determine the molecular formula. It outlines the step-by-step processes for performing mole calculations and conversions between grams, moles, molecules and volume. Practice problems are provided for calculating molar masses, determining moles from mass, calculating empirical formulas from elemental analysis, and determining molecular formulas from empirical formulas and molar masses.
This document is a transcript from a video lecture on chemistry topics for an AP Chemistry class. It covers objectives, questions, and content on stoichiometry, the mole concept, dimensional analysis, moles and particles, balancing chemical reactions, solubility rules, and writing net ionic equations. The instructor provides examples and practice problems for students to work through each concept. Students are given objectives for what they should know before and after each section. The overarching topics covered include the mole, stoichiometry calculations, balancing and classifying reactions, and writing balanced and net ionic equations.
Similar to HOW TO LEARN AND MASTER STOICHIOMETRY.pptx (20)
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
environment for investigating the changes in vegetation cover dynamics. Our study utilizes
advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
these activities. As the most crucial natural resource, its utilization by humans results in different
'Land uses,' which are determined by both human activities and the physical characteristics of the
land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
to significant land degradation, adversely affecting the region's land cover.
Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
cover is essential for various planning and management tasks related to the Earth's surface,
providing crucial environmental data for scientific, resource management, policy purposes, and
diverse human activities.
Accurate understanding of land use and cover is imperative for the development planning
of any area. Consequently, a wide range of professionals, including earth system scientists, land
and water managers, and urban planners, are interested in obtaining data on land use and cover
changes, conversion trends, and other related patterns. The spatial dimensions of land use and
cover support policymakers and scientists in making well-informed decisions, as alterations in
these patterns indicate shifts in economic and social conditions. Monitoring such changes with the
help of Advanced technologies like Remote Sensing and Geographic Information Systems is
crucial for coordinated efforts across different administrative levels. Advanced technologies like
Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
occur natural.
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
-------------------------------------------------------------------------------
Find out more about ISO training and certification services
Training: ISO/IEC 27001 Information Security Management System - EN | PECB
ISO/IEC 42001 Artificial Intelligence Management System - EN | PECB
General Data Protection Regulation (GDPR) - Training Courses - EN | PECB
Webinars: https://pecb.com/webinars
Article: https://pecb.com/article
-------------------------------------------------------------------------------
For more information about PECB:
Website: https://pecb.com/
LinkedIn: https://www.linkedin.com/company/pecb/
Facebook: https://www.facebook.com/PECBInternational/
Slideshare: http://www.slideshare.net/PECBCERTIFICATION
This slide is special for master students (MIBS & MIFB) in UUM. Also useful for readers who are interested in the topic of contemporary Islamic banking.
Main Java[All of the Base Concepts}.docxadhitya5119
This is part 1 of my Java Learning Journey. This Contains Custom methods, classes, constructors, packages, multithreading , try- catch block, finally block and more.
Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
"Learn about all the ways Walmart supports nonprofit organizations.
You will hear from Liz Willett, the Head of Nonprofits, and hear about what Walmart is doing to help nonprofits, including Walmart Business and Spark Good. Walmart Business+ is a new offer for nonprofits that offers discounts and also streamlines nonprofits order and expense tracking, saving time and money.
The webinar may also give some examples on how nonprofits can best leverage Walmart Business+.
The event will cover the following::
Walmart Business + (https://business.walmart.com/plus) is a new shopping experience for nonprofits, schools, and local business customers that connects an exclusive online shopping experience to stores. Benefits include free delivery and shipping, a 'Spend Analytics” feature, special discounts, deals and tax-exempt shopping.
Special TechSoup offer for a free 180 days membership, and up to $150 in discounts on eligible orders.
Spark Good (walmart.com/sparkgood) is a charitable platform that enables nonprofits to receive donations directly from customers and associates.
Answers about how you can do more with Walmart!"
This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.
How to Fix the Import Error in the Odoo 17Celine George
An import error occurs when a program fails to import a module or library, disrupting its execution. In languages like Python, this issue arises when the specified module cannot be found or accessed, hindering the program's functionality. Resolving import errors is crucial for maintaining smooth software operation and uninterrupted development processes.
A review of the growth of the Israel Genealogy Research Association Database Collection for the last 12 months. Our collection is now passed the 3 million mark and still growing. See which archives have contributed the most. See the different types of records we have, and which years have had records added. You can also see what we have for the future.
89. Remember this quote:
“In any field of learning, mastery is
said to be achieved only when there
is the correct recognition and
handling of all the patterns that
characterize that field.”
-Temple Eke
126. The Author
Temple Eke has been an active teacher of
Chemistry, Mathematics, Physics, and Biology
for over 30 years, helping thousands of
students excel in their various careers. He is
the author of over 40 books in Mathematics,
Physics, Biology, and Chemistry. He is well
known for his simplified teaching technique
and explicit writing style.