The document discusses reaction rates, equilibrium, and kinetics in chemistry. It defines kinetics as the study of reaction rates. Collision theory states that for a reaction to occur upon collision, the collision must be correct in orientation and energy. Factors like concentration, temperature, surface area, and catalysts affect reaction rates. Equilibrium is established when the forward and reverse reaction rates are equal. The equilibrium constant expression shows the ratio of products to reactants at equilibrium. The reaction quotient can be used to determine if a system is at equilibrium by comparing it to the equilibrium constant.
This document summarizes key concepts relating to reaction rates, equilibrium, and factors that affect them. It defines kinetics, reaction rates, and activation energy. It explains collision theory, reaction coordinate diagrams, and how equilibrium is established over time as the forward and reverse reactions proceed. It also defines equilibrium constants, reaction quotients, and Le Chatelier's principle. It lists factors that affect reaction rates like surface area, concentration, and temperature. Finally, it summarizes how changing conditions like concentration, temperature, and pressure can shift the position of equilibrium according to Le Chatelier's principle.
This document provides an overview of key concepts in equilibrium chemistry including reversible reactions, equilibrium constants, Le Chatelier's principle, and techniques for solving equilibrium problems using ICE charts and calculating reaction quotients. It defines equilibrium as a state where the rates of the forward and reverse reactions are equal. ICE charts are introduced as a method to organize information about initial concentrations, changes, and equilibrium concentrations in solving equilibrium problems. The document also discusses writing and using equilibrium constant expressions, solubility products, and reaction quotients to determine if a system is at equilibrium or not.
This document provides an overview of chemical equilibrium including:
- The law of mass action and how equilibrium is reached through forward and reverse reactions.
- Factors that affect equilibrium position including concentration, pressure, temperature, and catalyst addition based on Le Chatelier's principle.
- Applications of the equilibrium constant including predicting reaction direction and extent.
- Industrial uses of equilibrium concepts such as the Haber process for ammonia synthesis which applies pressure, temperature and product removal.
Chem 2 - Chemical Equilibrium VIII: Le Chatelier's Principle- Concepts and Re...Lumen Learning
This document discusses Le Chatelier's principle, which predicts how a chemical equilibrium will respond to changes in conditions. It defines a "stress" as any factor that disrupts equilibrium. Le Chatelier's principle states that if a system at equilibrium experiences a stress, the equilibrium will shift in a direction that counteracts the stress. Examples of stresses include adding or removing reactants/products, changing pressure or volume, and changing temperature. If more reactant is added, the reaction will shift towards making more products to use up the excess reactant.
This document discusses chemical equilibria, including definitions, the equilibrium constant Kc, and Le Chatelier's principle. It notes that chemical equilibrium occurs in a closed system where the rates of the forward and reverse reactions are equal. The equilibrium constant Kc relates the concentrations of products and reactants at equilibrium. Le Chatelier's principle states that if a system at equilibrium experiences a change or disturbance, the equilibrium will shift in a direction that counteracts the change.
Le Chatelier's Principle describes how chemical equilibriums respond to changes in conditions. When volume decreases, pressure increases, so the equilibrium shifts to reduce pressure by producing more products from fewer reactants. When temperature increases, the equilibrium shifts to absorb the extra heat by moving left to favor the endothermic reaction of reactants forming products.
This document discusses key concepts in chemical reactions and equations. It defines different types of chemical reactions like single displacement, synthesis, and decomposition reactions. It also explains important laws like the law of conservation of energy and mass. It defines exothermic and endothermic reactions as well as concepts like activation energy, catalysts, and inhibitors. Finally, it provides steps for balancing chemical equations.
The document discusses chemical equilibrium and Le Chatelier's principle. It explains that chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain unchanged. Le Chatelier's principle states that if a system at equilibrium experiences a change in concentration, temperature, or pressure, the equilibrium will shift to counteract the applied stress. The document provides examples of how changing temperature, concentration, or pressure would cause the equilibrium of a reaction to shift left or right.
This document summarizes key concepts relating to reaction rates, equilibrium, and factors that affect them. It defines kinetics, reaction rates, and activation energy. It explains collision theory, reaction coordinate diagrams, and how equilibrium is established over time as the forward and reverse reactions proceed. It also defines equilibrium constants, reaction quotients, and Le Chatelier's principle. It lists factors that affect reaction rates like surface area, concentration, and temperature. Finally, it summarizes how changing conditions like concentration, temperature, and pressure can shift the position of equilibrium according to Le Chatelier's principle.
This document provides an overview of key concepts in equilibrium chemistry including reversible reactions, equilibrium constants, Le Chatelier's principle, and techniques for solving equilibrium problems using ICE charts and calculating reaction quotients. It defines equilibrium as a state where the rates of the forward and reverse reactions are equal. ICE charts are introduced as a method to organize information about initial concentrations, changes, and equilibrium concentrations in solving equilibrium problems. The document also discusses writing and using equilibrium constant expressions, solubility products, and reaction quotients to determine if a system is at equilibrium or not.
This document provides an overview of chemical equilibrium including:
- The law of mass action and how equilibrium is reached through forward and reverse reactions.
- Factors that affect equilibrium position including concentration, pressure, temperature, and catalyst addition based on Le Chatelier's principle.
- Applications of the equilibrium constant including predicting reaction direction and extent.
- Industrial uses of equilibrium concepts such as the Haber process for ammonia synthesis which applies pressure, temperature and product removal.
Chem 2 - Chemical Equilibrium VIII: Le Chatelier's Principle- Concepts and Re...Lumen Learning
This document discusses Le Chatelier's principle, which predicts how a chemical equilibrium will respond to changes in conditions. It defines a "stress" as any factor that disrupts equilibrium. Le Chatelier's principle states that if a system at equilibrium experiences a stress, the equilibrium will shift in a direction that counteracts the stress. Examples of stresses include adding or removing reactants/products, changing pressure or volume, and changing temperature. If more reactant is added, the reaction will shift towards making more products to use up the excess reactant.
This document discusses chemical equilibria, including definitions, the equilibrium constant Kc, and Le Chatelier's principle. It notes that chemical equilibrium occurs in a closed system where the rates of the forward and reverse reactions are equal. The equilibrium constant Kc relates the concentrations of products and reactants at equilibrium. Le Chatelier's principle states that if a system at equilibrium experiences a change or disturbance, the equilibrium will shift in a direction that counteracts the change.
Le Chatelier's Principle describes how chemical equilibriums respond to changes in conditions. When volume decreases, pressure increases, so the equilibrium shifts to reduce pressure by producing more products from fewer reactants. When temperature increases, the equilibrium shifts to absorb the extra heat by moving left to favor the endothermic reaction of reactants forming products.
This document discusses key concepts in chemical reactions and equations. It defines different types of chemical reactions like single displacement, synthesis, and decomposition reactions. It also explains important laws like the law of conservation of energy and mass. It defines exothermic and endothermic reactions as well as concepts like activation energy, catalysts, and inhibitors. Finally, it provides steps for balancing chemical equations.
The document discusses chemical equilibrium and Le Chatelier's principle. It explains that chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain unchanged. Le Chatelier's principle states that if a system at equilibrium experiences a change in concentration, temperature, or pressure, the equilibrium will shift to counteract the applied stress. The document provides examples of how changing temperature, concentration, or pressure would cause the equilibrium of a reaction to shift left or right.
Henry Louis Le Châtelier, a French scientist, developed Le Châtelier's principle which states that if a system at equilibrium experiences a change in concentration, temperature, or pressure, the equilibrium will shift to counteract the change and re-establish equilibrium. The document discusses Le Châtelier's principle and how chemical equilibriums respond to changes in concentration, pressure, temperature, catalyst addition, and inert gas addition. Examples are provided to illustrate how the equilibrium shifts under different conditions according to Le Châtelier's principle.
Chem 2 - Chemical Equilibrium IX: Le Chatelier's Principle and Pressure - Vol...Lumen Learning
This document discusses how chemical equilibriums respond to changes in pressure, volume, and the addition of inert gases according to Le Chatelier's principle. It explains that when pressure increases on a system, the equilibrium shifts toward the direction with fewer moles of gas. When an inert gas is added at constant volume, the equilibrium does not shift, but when added at constant pressure the equilibrium shifts toward more moles of gas as the volume expands. The document uses examples and questions to illustrate these concepts.
1) The rate of a chemical reaction depends on factors like temperature, concentration, particle size, and the use of catalysts. Increasing temperature or concentration generally increases the reaction rate.
2) According to collision theory, particles must collide with sufficient kinetic energy, known as the activation energy, to react. Catalysts lower the activation energy needed for reactions.
3) For reversible reactions, an equilibrium is reached when the rates of the forward and reverse reactions are equal. Equilibrium can be influenced by changing concentrations, temperature, or pressure based on Le Chatelier's principle.
This document provides an overview of key concepts related to chemical equilibrium. It defines reversible reactions and explains that chemical equilibrium is reached when the rates of the forward and reverse reactions are equal, resulting in no further change in reactant and product concentrations over time. The document also discusses homogeneous and heterogeneous equilibrium, factors that affect equilibrium such as temperature, pressure, and concentration, Le Chatelier's principle, and examples of industrial processes that utilize chemical equilibrium concepts.
The document discusses the concept of chemical equilibrium. It explains that a system at equilibrium is in a balanced state where the forward and reverse reactions are occurring at equal rates, resulting in constant concentrations. It then addresses several questions: (1) the concentration of a gas at equilibrium does not change; (2) both condensation and vaporization occur at the same rate for a liquid-gas system; (3) conditions like closed container, stable temperature, and low activation energy are required for equilibrium. The document proceeds to describe Le Chatelier's principle, explaining how changing conditions like concentration, pressure, and temperature will cause the equilibrium to shift in order to counteract the applied stress.
Chemical equations must be balanced to obey the law of conservation of mass. This law states that matter is neither created nor destroyed in a chemical reaction, only transformed. To balance an equation, one counts the number of atoms of each element on both sides of the reaction. If the numbers are not equal, coefficients are placed in front of formulas to balance the atoms. For example, the equation H2 + Cl2 → HCl is balanced by adding a coefficient of 2 in front of HCl to make the chlorine atoms equal on both sides of the reaction. Balancing chemical equations ensures the law of conservation of mass is followed.
Chem 2 - Chemical Equilibrium IV: The Properties of the Equilibrium Constant ...Lumen Learning
This document discusses three properties of equilibrium constants:
1) If a reaction is reversed, the new equilibrium constant K is the inverse of the original value.
2) If two reactions are added together, the new equilibrium constant K is the product of the individual constants.
3) If reaction coefficients are multiplied by a factor, the new K is the original K raised to the power of that factor.
Examples are provided to illustrate applying these properties to calculate new equilibrium constants based on original values and how reactions are modified.
Chem 2 - Chemical Equilibrium VII: The Reaction Quotient Q for Non-equilbrium...Lumen Learning
This document discusses the reaction quotient Q and how it can be used to determine if a chemical reaction is at equilibrium or not. It explains that Q is calculated the same way as the equilibrium constant K, but Q can be calculated for any reaction conditions, while K only applies at equilibrium. If Q equals K, the reaction is at equilibrium. If Q is greater than K, there are too many products and the reaction will shift towards the reactants. If Q is less than K, there are too many reactants and the reaction will shift towards the products. An example problem demonstrates calculating Q and comparing it to K to determine the direction a reaction needs to shift.
Chem 2 - Chemical Equilibrium V: ICE Tables and Equilibrium CalculationsLumen Learning
This document discusses using ICE tables and the equilibrium constant expression to calculate equilibrium concentrations or partial pressures for a chemical reaction. It provides an example problem working through setting up an ICE table, filling in values, solving the equilibrium constant expression as a quadratic equation to find the change value x, and substituting x back into the ICE table and expression to determine the equilibrium partial pressures. The key steps are setting up the ICE table with initial, change, and equilibrium lines; using the equilibrium constant expression to set up an equation in terms of x; solving for x; and checking that substituting the calculated values back into the expression gives the known value of K.
The document discusses activation energy and the Arrhenius equation. It defines activation energy as the minimum amount of energy required for a chemical reaction to occur. The Arrhenius equation relates temperature, activation energy, and the rate constant of a reaction. The document then summarizes an experiment that demonstrates how reaction rate increases with temperature by measuring four reactions at different temperatures and constructing an Arrhenius plot from the results.
Le Chatelier's Principle states that if conditions of a system at equilibrium are changed, the equilibrium will shift to counteract the imposed change. Specifically:
- Increasing the concentration of a reactant will shift the equilibrium towards products.
- Decreasing the concentration of a reactant will shift equilibrium towards reactants.
- Increasing pressure of a gaseous reaction will shift equilibrium towards the side with fewer moles of gas.
- Increasing temperature of an endothermic reaction shifts equilibrium towards reactants, while an exothermic reaction shifts towards products.
1. Le Châtelier's principle states that if a system at equilibrium is disturbed by changing conditions, it will shift in a way to counteract the change and restore equilibrium.
2. Specifically, the document discusses how equilibrium shifts in response to changes in concentration of reactants/products, pressure on the system, addition of inert gases, presence of catalysts, and temperature.
3. Across examples of different chemical reactions, the document demonstrates that equilibrium always shifts in a direction that consumes any substance added in excess or replaces any substance removed, relieves pressure increases, and offsets temperature changes to reestablish equilibrium.
The document discusses chemical equilibrium. It begins by defining chemical equilibrium as a dynamic state where the rates of the forward and reverse reactions are equal, such that there is no net change in concentrations. It then discusses concepts such as the equilibrium constant K, reaction quotient Q, Le Chatelier's principle, and factors that affect equilibrium like concentration, pressure, temperature, and catalysts. In summary, (1) chemical equilibrium is a dynamic state with equal forward and reverse reaction rates, (2) the equilibrium constant K relates concentrations at equilibrium, and (3) systems at equilibrium will shift in response to changes to reduce stress and reestablish equilibrium.
Le Châtelier's Principle states that if a stress is applied to a system at equilibrium, the system will adjust to partially counteract the stress and reach a new equilibrium position. Changes in concentration, pressure, volume, or temperature can act as stresses. For example, increasing the concentration of reactants will shift the equilibrium to the product side. A catalyst will speed the rate of both the forward and reverse reactions but will not change the equilibrium position or constant.
3rd Lecture on Chemical Equilibrium | Chemistry Part II | 11th StdAnsari Usama
The document discusses Le Chatelier's principle and how various factors affect chemical equilibrium. It explains that if a stress is applied to a system at equilibrium, the system will respond in a way to minimize the effect. The factors discussed are concentration, pressure, temperature, and catalysts. An example of the industrial Haber process for ammonia synthesis is provided to demonstrate the application of Le Chatelier's principle.
Collision theory and transition state theorynargis aman
Transition state theory provides an alternate approach to calculating reaction rates. It postulates that reactions proceed via an activated complex or transition state that is in equilibrium with the reactants. The rate of reaction is directly proportional to the concentration of the activated complex times the frequency at which the complex dissociates to form products. The entropy of activation gives the extent to which the transition state is more disordered compared to the starting materials, and can be used to interpret the pre-exponential factor in the Arrhenius equation.
Lect w6 152_abbrev_ le chatelier and calculations_1_algchelss
This document provides an overview of key concepts from a general chemistry unit on chemical equilibrium. It introduces the reaction quotient Q and how it relates to the equilibrium constant K. It discusses how changing conditions like concentration, pressure, volume, and temperature can shift an equilibrium position according to Le Châtelier's principle. Examples are provided for writing reaction quotients, determining if a reaction is at equilibrium, and calculating equilibrium concentrations. Approximations are described for simplifying equilibrium calculations when concentrations differ greatly from K values.
This document provides guidance on generating "how-might-we" questions to address a design challenge from a specific point of view. It outlines challenges such as redesigning the airport ground experience from the perspective of a harried mother traveling with four playful children. It then lists techniques for developing how-might-we questions that retain the unique perspective, such as removing problems, exploring alternatives, questioning assumptions, utilizing unexpected resources, creating analogies, or changing the status quo.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive function. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
This document provides an overview of chemical equilibrium concepts for an AP Chemistry course. It begins with definitions of equilibrium, dynamic equilibrium, and equilibrium constants. It then discusses how to write equilibrium constant expressions and calculate equilibrium constants. The document also covers reaction quotients, solubility equilibrium constants, and using ICE charts to solve equilibrium problems. The key information presented includes the concepts of reversible reactions reaching dynamic equilibrium when the forward and reverse reaction rates are equal, and that the equilibrium constant expression is the ratio of product to reactant concentrations raised to their balanced equation coefficients.
This document provides an overview of key concepts and formulas for kinematics in one dimension, including definitions of distance, displacement, speed, velocity, acceleration, and other related terms. It lists important formulas such as the equations for velocity, acceleration, displacement, and final velocity. Diagrams illustrate the differences between constant velocity and constant acceleration motion. The document concludes with tips for solving kinematics problems, including an example of calculating the time for a book to fall from a shelf.
Students at Banta School were having issues with squirrels digging holes in the school playground, which were causing injuries. The students decided to address this problem by designing a new habitat on school grounds to attract the squirrels away from the playground. They researched what squirrels need in a habitat and created plans for a "squirrel park" with the right plants, structures, water, and soil. The students then built the habitat and monitored it to see if the squirrels began using it instead of the playground. Over time they observed the squirrels and gathered data on how many were using the new habitat versus the playground. The project allowed students to develop solutions using engineering design and address a real environmental issue through collaboration.
Henry Louis Le Châtelier, a French scientist, developed Le Châtelier's principle which states that if a system at equilibrium experiences a change in concentration, temperature, or pressure, the equilibrium will shift to counteract the change and re-establish equilibrium. The document discusses Le Châtelier's principle and how chemical equilibriums respond to changes in concentration, pressure, temperature, catalyst addition, and inert gas addition. Examples are provided to illustrate how the equilibrium shifts under different conditions according to Le Châtelier's principle.
Chem 2 - Chemical Equilibrium IX: Le Chatelier's Principle and Pressure - Vol...Lumen Learning
This document discusses how chemical equilibriums respond to changes in pressure, volume, and the addition of inert gases according to Le Chatelier's principle. It explains that when pressure increases on a system, the equilibrium shifts toward the direction with fewer moles of gas. When an inert gas is added at constant volume, the equilibrium does not shift, but when added at constant pressure the equilibrium shifts toward more moles of gas as the volume expands. The document uses examples and questions to illustrate these concepts.
1) The rate of a chemical reaction depends on factors like temperature, concentration, particle size, and the use of catalysts. Increasing temperature or concentration generally increases the reaction rate.
2) According to collision theory, particles must collide with sufficient kinetic energy, known as the activation energy, to react. Catalysts lower the activation energy needed for reactions.
3) For reversible reactions, an equilibrium is reached when the rates of the forward and reverse reactions are equal. Equilibrium can be influenced by changing concentrations, temperature, or pressure based on Le Chatelier's principle.
This document provides an overview of key concepts related to chemical equilibrium. It defines reversible reactions and explains that chemical equilibrium is reached when the rates of the forward and reverse reactions are equal, resulting in no further change in reactant and product concentrations over time. The document also discusses homogeneous and heterogeneous equilibrium, factors that affect equilibrium such as temperature, pressure, and concentration, Le Chatelier's principle, and examples of industrial processes that utilize chemical equilibrium concepts.
The document discusses the concept of chemical equilibrium. It explains that a system at equilibrium is in a balanced state where the forward and reverse reactions are occurring at equal rates, resulting in constant concentrations. It then addresses several questions: (1) the concentration of a gas at equilibrium does not change; (2) both condensation and vaporization occur at the same rate for a liquid-gas system; (3) conditions like closed container, stable temperature, and low activation energy are required for equilibrium. The document proceeds to describe Le Chatelier's principle, explaining how changing conditions like concentration, pressure, and temperature will cause the equilibrium to shift in order to counteract the applied stress.
Chemical equations must be balanced to obey the law of conservation of mass. This law states that matter is neither created nor destroyed in a chemical reaction, only transformed. To balance an equation, one counts the number of atoms of each element on both sides of the reaction. If the numbers are not equal, coefficients are placed in front of formulas to balance the atoms. For example, the equation H2 + Cl2 → HCl is balanced by adding a coefficient of 2 in front of HCl to make the chlorine atoms equal on both sides of the reaction. Balancing chemical equations ensures the law of conservation of mass is followed.
Chem 2 - Chemical Equilibrium IV: The Properties of the Equilibrium Constant ...Lumen Learning
This document discusses three properties of equilibrium constants:
1) If a reaction is reversed, the new equilibrium constant K is the inverse of the original value.
2) If two reactions are added together, the new equilibrium constant K is the product of the individual constants.
3) If reaction coefficients are multiplied by a factor, the new K is the original K raised to the power of that factor.
Examples are provided to illustrate applying these properties to calculate new equilibrium constants based on original values and how reactions are modified.
Chem 2 - Chemical Equilibrium VII: The Reaction Quotient Q for Non-equilbrium...Lumen Learning
This document discusses the reaction quotient Q and how it can be used to determine if a chemical reaction is at equilibrium or not. It explains that Q is calculated the same way as the equilibrium constant K, but Q can be calculated for any reaction conditions, while K only applies at equilibrium. If Q equals K, the reaction is at equilibrium. If Q is greater than K, there are too many products and the reaction will shift towards the reactants. If Q is less than K, there are too many reactants and the reaction will shift towards the products. An example problem demonstrates calculating Q and comparing it to K to determine the direction a reaction needs to shift.
Chem 2 - Chemical Equilibrium V: ICE Tables and Equilibrium CalculationsLumen Learning
This document discusses using ICE tables and the equilibrium constant expression to calculate equilibrium concentrations or partial pressures for a chemical reaction. It provides an example problem working through setting up an ICE table, filling in values, solving the equilibrium constant expression as a quadratic equation to find the change value x, and substituting x back into the ICE table and expression to determine the equilibrium partial pressures. The key steps are setting up the ICE table with initial, change, and equilibrium lines; using the equilibrium constant expression to set up an equation in terms of x; solving for x; and checking that substituting the calculated values back into the expression gives the known value of K.
The document discusses activation energy and the Arrhenius equation. It defines activation energy as the minimum amount of energy required for a chemical reaction to occur. The Arrhenius equation relates temperature, activation energy, and the rate constant of a reaction. The document then summarizes an experiment that demonstrates how reaction rate increases with temperature by measuring four reactions at different temperatures and constructing an Arrhenius plot from the results.
Le Chatelier's Principle states that if conditions of a system at equilibrium are changed, the equilibrium will shift to counteract the imposed change. Specifically:
- Increasing the concentration of a reactant will shift the equilibrium towards products.
- Decreasing the concentration of a reactant will shift equilibrium towards reactants.
- Increasing pressure of a gaseous reaction will shift equilibrium towards the side with fewer moles of gas.
- Increasing temperature of an endothermic reaction shifts equilibrium towards reactants, while an exothermic reaction shifts towards products.
1. Le Châtelier's principle states that if a system at equilibrium is disturbed by changing conditions, it will shift in a way to counteract the change and restore equilibrium.
2. Specifically, the document discusses how equilibrium shifts in response to changes in concentration of reactants/products, pressure on the system, addition of inert gases, presence of catalysts, and temperature.
3. Across examples of different chemical reactions, the document demonstrates that equilibrium always shifts in a direction that consumes any substance added in excess or replaces any substance removed, relieves pressure increases, and offsets temperature changes to reestablish equilibrium.
The document discusses chemical equilibrium. It begins by defining chemical equilibrium as a dynamic state where the rates of the forward and reverse reactions are equal, such that there is no net change in concentrations. It then discusses concepts such as the equilibrium constant K, reaction quotient Q, Le Chatelier's principle, and factors that affect equilibrium like concentration, pressure, temperature, and catalysts. In summary, (1) chemical equilibrium is a dynamic state with equal forward and reverse reaction rates, (2) the equilibrium constant K relates concentrations at equilibrium, and (3) systems at equilibrium will shift in response to changes to reduce stress and reestablish equilibrium.
Le Châtelier's Principle states that if a stress is applied to a system at equilibrium, the system will adjust to partially counteract the stress and reach a new equilibrium position. Changes in concentration, pressure, volume, or temperature can act as stresses. For example, increasing the concentration of reactants will shift the equilibrium to the product side. A catalyst will speed the rate of both the forward and reverse reactions but will not change the equilibrium position or constant.
3rd Lecture on Chemical Equilibrium | Chemistry Part II | 11th StdAnsari Usama
The document discusses Le Chatelier's principle and how various factors affect chemical equilibrium. It explains that if a stress is applied to a system at equilibrium, the system will respond in a way to minimize the effect. The factors discussed are concentration, pressure, temperature, and catalysts. An example of the industrial Haber process for ammonia synthesis is provided to demonstrate the application of Le Chatelier's principle.
Collision theory and transition state theorynargis aman
Transition state theory provides an alternate approach to calculating reaction rates. It postulates that reactions proceed via an activated complex or transition state that is in equilibrium with the reactants. The rate of reaction is directly proportional to the concentration of the activated complex times the frequency at which the complex dissociates to form products. The entropy of activation gives the extent to which the transition state is more disordered compared to the starting materials, and can be used to interpret the pre-exponential factor in the Arrhenius equation.
Lect w6 152_abbrev_ le chatelier and calculations_1_algchelss
This document provides an overview of key concepts from a general chemistry unit on chemical equilibrium. It introduces the reaction quotient Q and how it relates to the equilibrium constant K. It discusses how changing conditions like concentration, pressure, volume, and temperature can shift an equilibrium position according to Le Châtelier's principle. Examples are provided for writing reaction quotients, determining if a reaction is at equilibrium, and calculating equilibrium concentrations. Approximations are described for simplifying equilibrium calculations when concentrations differ greatly from K values.
This document provides guidance on generating "how-might-we" questions to address a design challenge from a specific point of view. It outlines challenges such as redesigning the airport ground experience from the perspective of a harried mother traveling with four playful children. It then lists techniques for developing how-might-we questions that retain the unique perspective, such as removing problems, exploring alternatives, questioning assumptions, utilizing unexpected resources, creating analogies, or changing the status quo.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive function. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
This document provides an overview of chemical equilibrium concepts for an AP Chemistry course. It begins with definitions of equilibrium, dynamic equilibrium, and equilibrium constants. It then discusses how to write equilibrium constant expressions and calculate equilibrium constants. The document also covers reaction quotients, solubility equilibrium constants, and using ICE charts to solve equilibrium problems. The key information presented includes the concepts of reversible reactions reaching dynamic equilibrium when the forward and reverse reaction rates are equal, and that the equilibrium constant expression is the ratio of product to reactant concentrations raised to their balanced equation coefficients.
This document provides an overview of key concepts and formulas for kinematics in one dimension, including definitions of distance, displacement, speed, velocity, acceleration, and other related terms. It lists important formulas such as the equations for velocity, acceleration, displacement, and final velocity. Diagrams illustrate the differences between constant velocity and constant acceleration motion. The document concludes with tips for solving kinematics problems, including an example of calculating the time for a book to fall from a shelf.
Students at Banta School were having issues with squirrels digging holes in the school playground, which were causing injuries. The students decided to address this problem by designing a new habitat on school grounds to attract the squirrels away from the playground. They researched what squirrels need in a habitat and created plans for a "squirrel park" with the right plants, structures, water, and soil. The students then built the habitat and monitored it to see if the squirrels began using it instead of the playground. Over time they observed the squirrels and gathered data on how many were using the new habitat versus the playground. The project allowed students to develop solutions using engineering design and address a real environmental issue through collaboration.
This document appears to be a table for an AP Physics experiment recording trial numbers, angle measurements, distances, masses, and elevations for 10 trials. The document also has a section to record observations from the experiment.
This document provides an overview of key concepts in animal function for AP Biology, including definitions of 20 terms related to digestion, respiration, circulation, defense, reproduction, sensory and signal transmission, and the nervous system. It describes the main stages and components of digestion in the stomach and small intestine, respiration in the lungs, and the pulmonary and systemic circuits of circulation. It also outlines nonspecific and specific immune defenses, the three germ layers formed during gastrulation, and how sensory stimuli are transmitted via receptors, neurons and synapses to effectors. A diagram labels the major structures and blood flow pathways in the human circulatory system.
There are four main types of animal tissues: muscular, nervous, connective, and epithelial tissue. Muscular tissue includes skeletal, smooth, and cardiac muscle. Nervous tissue contains neurons and glial cells that help conduct electrical signals. Connective tissue includes several types that provide binding, support, protection and storage functions. Epithelial tissue has cell shapes and layers that act as barriers and aid movement of materials. The document then lists and briefly describes the 11 major organ systems in animals and their functions, including the muscular, digestive, respiratory, cardiovascular, lymphatic, excretory, endocrine, reproductive, nervous, skeletal and skin systems.
The document provides an overview of the key topics covered on the AP Physics B exam, including Newton's Laws, wave motion, optics, the photoelectric effect, electromagnetism, and atomic physics. It emphasizes that the exam evaluates students' understanding of core physics concepts as well as their ability to show work clearly in free response questions using correct equations, values, units, and significant figures. The multiple choice section requires calculating without a calculator.
This document provides an overview of problem-solving strategies and techniques for physics exams. It outlines a 5-step general problem-solving strategy of identifying known and unknown information, selecting a strategy, applying the strategy, and reviewing the answer. Mnemonic devices and the KUDOS method for word problems are also described. The document concludes with exam preparation and taking tips, such as staying ahead, making a cheat sheet, understanding question formats, and showing work.
The key events in speciation are the isolation of a population's gene pool, which can occur through external barriers like geographic separation, or internal barriers that develop later. External barriers initially isolate populations, exposing them to different environments where natural selection can cause adaptations. Over time, internal barriers to reproduction may form as a byproduct and further maintain genetic isolation between the species. Sympatric speciation differs in that internal barriers form first without an initial external cause, often through chromosome changes making organisms unable to mate.
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.
This document provides key biology terms and concepts related to evolutionary history. It discusses endosymbiotic theory, which proposes that mitochondria and chloroplasts originated from ancient endosymbiotic relationships between bacteria and larger prokaryotic cells. It also describes paedogenesis, the process by which some larval chordates reached sexual maturity without undergoing complete metamorphosis, and how this may have led to modifications in chordate traits. Several major extinction events are noted, including one at the Triassic period where 90% of animal species went extinct, possibly due to asteroid impact. The document outlines the basic sequence of events that may have led to the emergence of early life forms and discusses challenges with using the fossil record to
The document summarizes key concepts about the evolution of animal diversity. It describes the major splits in animal evolution including acoelomates vs coelomates, radiates vs bilateria, and protosomes vs deuterosomes. The Cambrian explosion occurred around 500 million years ago, resulting in the emergence of modern animal phyla. Today's animals can be classified into over 35 phyla based on their adult forms, embryological development, body symmetry, and presence of tissues and body cavities. Examples of major phyla include sponges, cnidarians, flatworms, arthropods, mollusks, and chordates.
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 document provides an overview of key concepts and formulas relating to mechanics of solids and fluids in physics. It defines important terms like the different states of matter, density, pressure, stress and strain. It also outlines fundamental principles including Pascal's principle describing pressure variations in fluids, Archimedes' principle of buoyancy, and Bernoulli's equation relating pressure, velocity and height along a streamline. The document concludes by listing common variables and units used and some example formulas for topics like thermal expansion, stress, and fluid flow properties.
The document provides an overview of key biology terms and concepts including:
- Cells are the basic unit of life and different types of organisms get nutrients in different ways.
- Evolution and genes help explain how living things change over time and pass on traits.
- Homeostasis allows organisms to maintain stable internal conditions.
- There are various branches of biology that study different aspects of living things.
- Major theories in biology include the cell theory, theory of evolution, and gene theory.
- Organisms are classified into five kingdoms based on their characteristics.
This document provides an overview of key concepts in equilibrium chemistry including reversible reactions, equilibrium constants, Le Chatelier's principle, and techniques for solving equilibrium problems using ICE charts and determining solubility. It defines equilibrium as a state where the rates of the forward and reverse reactions are equal. ICE charts are introduced as a method to organize information about initial concentrations, changes, and equilibrium concentrations in solving equilibrium problems. The document also describes how to write equilibrium constant expressions, reaction quotient expressions, and solubility product expressions.
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 a summary of key biology terms and concepts related to evolution, including:
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- A description of the process of natural selection, including how random genetic variations, interaction with the environment, and differential reproductive success can lead to adaptation over time.
- A phylogenetic tree showing the evolutionary relationships between major primate groups like humans, chimpanzees, gorillas, orangutans, gibbons, and old and new world monkeys.
This document discusses chemical equilibrium, which occurs when the rate of the forward reaction equals the rate of the reverse reaction in a closed system. It defines the equilibrium constant (Kc) and explains that a high Kc value means a high product yield, while a low Kc means a low product yield. It also describes Le Chatelier's Principle, which states that applying stress to a system in equilibrium will cause the equilibrium to shift to reduce the effect of the stress, and discusses how temperature, concentration, and pressure influence the position and value of equilibrium constants.
F.Sc. Part 1 Chemistry.Ch.11.Test (Malik Xufyan)Malik Xufyan
This document contains information about Malik's Chemistry test series books for classes 9th, 10th, F.Sc part 1 and part 2. It provides chapter-wise and board paper-wise test series. It also mentions the publisher Jhang Institute for Advanced Studies and provides their contact details. The document contains the list of chapters and topics covered in the test series books along with their page numbers.
A complete introduction to all things chemical kinetics designed specifically for non-chemists to understand. Fair warning: The presentation is very rigorous in its mathematical treatment, which is makes it a useful reference for looking up equations, but this can unfortunately make it less polished and flowing then a typical presentation. I tried my best to spell everything out clearly, but despite my best efforts it's still pretty dense.
The document contains questions and answers related to chemical equilibrium. It defines terms like active mass, law of mass action, irreversible and reversible reactions, and chemical equilibrium. It also describes Le Chatelier's principle, stating that changing concentration, temperature, or pressure causes the equilibrium of a reaction to shift in the direction that counteracts the applied stress. Examples are provided to explain how increasing or decreasing temperature, pressure, or concentration affects the yield of products in endothermic and exothermic reactions.
The document discusses reaction rates and factors that affect them, including the nature of reactants, concentration of reactants, temperature, presence of a catalyst, and surface area. It describes collision theory and how it explains how these factors influence reaction rates. Different methods for measuring reaction rates are discussed depending on the type of product produced. The minimum energy required for reactions, known as activation energy, and how temperature and catalysts can provide energy to overcome this are also summarized.
Peter Waage and Cato Guldberg pioneered the development of chemical kinetics by formulating the law of mass action in 1864. Chemical kinetics is the study of reaction rates and factors that affect the rates, including concentration, temperature, catalysts, surface area, pressure, and mechanism. The rate of reaction is expressed as the change in reactants or products per unit time. Collision theory and transition state theory are two theories that describe reaction rates and mechanisms.
Chemical equilibrium: law of mass action, determination of equilibrium constant,
heterogeneous equilibrium and homogenous equilibrium, le chateliar principle and vant
hoff equation
1. The collision theory describes how chemical reactions occur through molecular collisions that meet specific criteria: molecules must collide with proper orientation and energy to react.
2. Chemical kinetics is the study of reaction rates and mechanisms, relying on experimental data. It describes how fast reactions occur through molecular collisions.
3. According to the collision theory, a chemical reaction takes place during an effective collision when reacting molecules collide with proper orientation and energy equal to or above the activation energy.
This document outlines the course contents, objectives, and topics for a Chemical Reaction Engineering course. The course will cover topics such as kinetics of homogeneous and heterogeneous reactions, reactor design including batch, mixed flow, plug flow, and catalytic reactors. Students will learn how to develop rate expressions and design industrial reactors by applying principles of thermodynamics and reaction kinetics. The objective is to provide an in-depth understanding of commonly used chemical reactor designs.
The document discusses collision theory and factors that affect chemical reaction rates. Collision theory states that for a reaction to occur, reactant particles must collide with enough kinetic energy to overcome the activation energy barrier and they must collide in the correct orientation. The rate of reaction depends on factors like activation energy, temperature, concentration, and surface area. A higher temperature, concentration, or surface area increases the collision rate of reactants and leads to more successful collisions and a faster reaction.
The document discusses chemical reactions, including definitions, examples of reactions shown in pictures, how to write chemical equations, and factors that affect the rate of reactions. It defines a chemical reaction as when molecules combine or break apart through collisions, outlines how to balance chemical equations by adjusting coefficients, and explains that temperature, concentration, surface area, and catalysts can impact the speed of reactions.
The document discusses the factors that affect the rate of chemical reactions, including temperature, concentration, surface area, and particle size. Chemical reactions occur when particles collide with sufficient energy to break bonds and proper orientation to form new bonds. The rate of reactions increases with higher temperatures, concentrations, and surface areas as these factors lead to more frequent and energetic collisions between particles.
The document discusses chemical equilibrium, which occurs when a reversible reaction reaches a state where the rates of the forward and reverse reactions are equal. It provides examples of reversible reactions using double-headed arrows and explains that at equilibrium, the concentrations of reactants and products remain constant. The document also discusses how equilibrium can be determined through techniques like titration and spectroscopy, and how the equilibrium constant Kc is calculated based on the concentrations of reactants and products in the balanced chemical equation.
chemical kinetics-kinetic vs thermodynamicFarhadAlsaeid
This document discusses the differences between chemical kinetics and thermodynamics. Thermodynamics deals with whether a reaction can occur based on energy changes and equilibrium, while kinetics is concerned with how fast reactions occur and the rates of change over time. The document provides examples of factors studied in kinetics like reaction mechanisms and rates. While thermodynamics determines reaction spontaneity based on free energy, kinetics is needed to understand how long reactions take to reach equilibrium and what factors influence reaction rates.
1. The document provides information about online chemistry homework help and solutions for entire courses, exams, and homework assignments.
2. It includes examples of chemistry problems and questions related to plotting calibration curves, determining empirical formulas, acid-base reactions, and more.
3. Users can purchase solutions to specific problems or full course help starting at $3-10 per question or topic.
1) The document provides links to purchase homework help and exam solutions in chemistry and other courses without needing to register. Subjects include general chemistry, organic chemistry, biochemistry, and chemical engineering.
2) Sample problems are provided and include questions about plotting a calibration curve from dilution data, determining the empirical and molecular formulas of allicin, identifying acids and bases in a neutralization reaction, and calculating the Ksp value of a precipitate.
3) Other links relate to chemistry lab assignments on topics like radiocarbon dating, Hess's law, saponification reactions, and more. Custom homework help and exam solutions are available for purchase for a variety of chemistry and other science courses.
1) The document provides links to purchase homework help and exam solutions in chemistry and other courses without needing to register. Subjects include general chemistry, organic chemistry, and chemistry labs.
2) Sample problems are provided and include questions about plotting a calibration curve from dilution data, determining the empirical and molecular formulas of allicin, identifying acids and bases in a neutralization reaction, and calculating the Ksp value of a precipitate formed.
3) Other links relate to chemistry concepts like radiocarbon dating, Hess's law, saponification reactions, and writing chemical equations. Payment amounts ranging from $3-$10 are listed next to each problem or concept area.
1) The document provides links to purchase homework help and exam solutions in chemistry and other courses without needing to register. Subjects include general chemistry, organic chemistry, and chemistry labs.
2) Sample problems are provided and include questions about plotting a calibration curve from dilution data, determining the empirical and molecular formulas of a compound, acid-base reactions, and equilibrium calculations.
3) Clicking the links would provide access to step-by-step solutions to homework problems, exams, and lab reports across various chemistry topics for purchase.
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This document provides additional practice problems for balancing oxidation-reduction reactions in acidic and basic solutions. The problems cover reactions involving silver, zinc, chromium, phosphorus, manganese, chlorine, iron, hydrogen peroxide, and copper species. Balanced equations are provided as answers for each reaction.
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Acids have a sour taste, are electrolytes, turn indicators red, and have a pH less than 7. They donate protons and can neutralize bases to form salts and water. Bases have a bitter taste, are electrolytes, turn indicators blue or yellow, and have a pH greater than 7. They accept protons and can neutralize acids to form salts and water. Common acids include nitric acid, hydrochloric acid, acetic acid, sulfuric acid, and phosphoric acid. Common bases include lithium hydroxide, sodium hydroxide, potassium hydroxide, magnesium hydroxide, and calcium hydroxide.
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This document provides the syllabus for the STEM 352: STEM 2 course offered at Teachers College of San Joaquin. The syllabus outlines the dates, times, instructor contact information, course description, learning outcomes, assignments, grading policy, schedule, and expectations for the course. The course focuses on examining STEM curriculum, active learning strategies, and student assessment. Students will learn STEM education pedagogy and make connections between STEM education and Common Core and NGSS standards. The syllabus provides the framework and requirements for students to develop skills in STEM curriculum design and instruction.
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