Chemical reactions
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This document discusses key concepts in chemistry including types of chemical reactions such as single displacement, synthesis, decomposition, and double displacement reactions. It also covers important laws like the law of conservation of energy and mass. Exothermic and endothermic reactions are defined as well as activation energy, catalysts, and inhibitors. The key components of a balanced chemical equation like reactants and products are outlined. Finally, the six steps for balancing chemical equations are provided.
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Chemical reactions
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.
Chapter 6 2
A chemical reaction involves one or more substances being changed into new substances. It consists of reactants that are transformed into products, as represented by a balanced chemical equation showing the rearrangement of atoms. For a reaction to occur, the reactants must absorb a minimum amount of energy called the activation energy. Reactions can be endothermic, absorbing heat, or exothermic, releasing heat. Catalysts lower the activation energy needed and speed up the reaction without being used up themselves. Enzymes are biological catalysts with an active site that binds to substrate reactants.
Factors that affect Reaction Rates
Chemical changes occur when substances combine to form new substances and are not reversible without further chemical reactions. The rate of a chemical reaction depends on factors like the nature of reactants, temperature, concentration, surface area, and presence of catalysts. A catalyst lowers the activation energy needed for molecules to collide and react, accelerating the reaction rate without being consumed in the process.
Energy and chemical change
The document discusses energy changes that occur during chemical reactions. It explains that energy is absorbed when bonds in reactants break and released when new bonds in products form. If the energy released is greater than the energy absorbed, the reaction is exothermic and releases heat. If energy absorbed is greater, the reaction is endothermic and absorbs heat. The heat of reaction, ΔH, is calculated as the energy of products minus reactants and is negative for exothermic reactions and positive for endothermic reactions. Activation energy is also defined as the minimum energy needed to start a chemical reaction.
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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.
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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.
Rate and extent of reaction
This document discusses reaction rates and factors that affect reaction rates. It explains that reaction rate is calculated based on the moles of product formed or reactants used over the reaction time. The rate of reaction is affected by properties of the reactants, concentration, surface area, pressure, temperature, and presence of a catalyst. Various methods can be used to measure reaction rates depending on the products, such as collecting gases, measuring precipitates, or observing color changes. For a reaction to occur, particles must collide with sufficient energy to overcome the activation energy, and increasing temperature or adding a catalyst can provide this energy. A catalyst lowers the activation energy and speeds up the reaction but remains unchanged after.
Thermodynamics
This document discusses several key concepts in thermodynamics and chemical kinetics:
1. Chemical reactions can proceed partially, producing some products but leaving some original reactants. The rate of reactions is affected by factors like temperature.
2. There are two types of energy - potential energy stored in a system and kinetic energy of motion. Bond formation releases energy while bond breaking absorbs energy.
3. The tendency of reactions to occur spontaneously can be predicted from the free energy change, determined by both entropy change and enthalpy change. Reaction rates depend on factors like activation energy, temperature, concentration, and presence of catalysts.
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Chemical reactions
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.
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A chemical reaction involves one or more substances being changed into new substances. It consists of reactants that are transformed into products, as represented by a balanced chemical equation showing the rearrangement of atoms. For a reaction to occur, the reactants must absorb a minimum amount of energy called the activation energy. Reactions can be endothermic, absorbing heat, or exothermic, releasing heat. Catalysts lower the activation energy needed and speed up the reaction without being used up themselves. Enzymes are biological catalysts with an active site that binds to substrate reactants.
Factors that affect Reaction Rates
Chemical changes occur when substances combine to form new substances and are not reversible without further chemical reactions. The rate of a chemical reaction depends on factors like the nature of reactants, temperature, concentration, surface area, and presence of catalysts. A catalyst lowers the activation energy needed for molecules to collide and react, accelerating the reaction rate without being consumed in the process.
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The document discusses energy changes that occur during chemical reactions. It explains that energy is absorbed when bonds in reactants break and released when new bonds in products form. If the energy released is greater than the energy absorbed, the reaction is exothermic and releases heat. If energy absorbed is greater, the reaction is endothermic and absorbs heat. The heat of reaction, ΔH, is calculated as the energy of products minus reactants and is negative for exothermic reactions and positive for endothermic reactions. Activation energy is also defined as the minimum energy needed to start a chemical reaction.
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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.
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This document discusses reaction rates and factors that affect reaction rates. It explains that reaction rate is calculated based on the moles of product formed or reactants used over the reaction time. The rate of reaction is affected by properties of the reactants, concentration, surface area, pressure, temperature, and presence of a catalyst. Various methods can be used to measure reaction rates depending on the products, such as collecting gases, measuring precipitates, or observing color changes. For a reaction to occur, particles must collide with sufficient energy to overcome the activation energy, and increasing temperature or adding a catalyst can provide this energy. A catalyst lowers the activation energy and speeds up the reaction but remains unchanged after.
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This document discusses several key concepts in thermodynamics and chemical kinetics:
1. Chemical reactions can proceed partially, producing some products but leaving some original reactants. The rate of reactions is affected by factors like temperature.
2. There are two types of energy - potential energy stored in a system and kinetic energy of motion. Bond formation releases energy while bond breaking absorbs energy.
3. The tendency of reactions to occur spontaneously can be predicted from the free energy change, determined by both entropy change and enthalpy change. Reaction rates depend on factors like activation energy, temperature, concentration, and presence of catalysts.
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Collisions between reactants are necessary for chemical reactions to occur. The reactants must collide with the proper orientation and with sufficient kinetic energy to overcome the activation energy barrier. Adding a catalyst can also increase the reaction rate by lowering the activation energy needed for collisions between reactants to be productive.
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Conventional transition state theory
1) Transition state theory (TST) explains reaction rates by assuming a special type of equilibrium between reactants and unstable transition state complexes that have partially formed bonds between reactants and products.
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Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) Curriculum
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Film vocab for eal 3 students: Australia the movie
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IGCSE Biology Chapter 14- Reproduction in Plants.pdf
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Bed Making ( Introduction, Purpose, Types, Articles, Scientific principles, N...
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Chapter wise All Notes of First year Basic Civil Engineering.pptx
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NEWSPAPERS - QUESTION 1 - REVISION POWERPOINT.pptx
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Walmart Business+ and Spark Good for Nonprofits.pdf
Chemical reactions
- 1. Chemical Reactions • Single displacement reaction – reaction in which one element take the place of another element in a compound • Synthesis reaction – reaction in which two or more substance combine to form a new substance • Decomposition reaction – reaction in which a single compound breaks down to form two or more simpler substances. • Double displacement reaction – reaction in which a gas, precipitate, or molecular compound forms from the exchange of ions between two compounds
- 2. Laws and Energy • Law of conservation of energy – the law that states that energy cannot be created or destroyed but can be changes from one form to another • Law of conservation of mass – law that states that mass cannot be created or destroyed in ordinary chemical or physical changes • Exothermic reactions – energy is released, usually in the form of heat • Endothermic reactions – energy is added, usually in the form of heat • Activation energy – minimum amount of energy needed to start a chemical reaction
- 3. • Catalyst – substance that changes the rate of a reaction without being used up or changed • Inhibitor – substance that can slow down or stop a chemical reaction
- 4. Parts of a Chemical Equation • Chemical equations consist of reactants (what you start with) and products (what you end up with) • Because of the laws of mass and energy, what you start with (reactants) must appear in what you end up with (products)
- 5. Steps to balance equations: 1. Separate the equation 2. List all elements on each side of the equation 3. Count the total number of atoms for each element 4. Find the first element that does not balance 5. ADD a coefficient to the front of the chemical formula for that element and recalculate the number of atoms in the equation 6. Repeat the process until the left side is equal to the right side of the equation