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Chemical reactions involve changes in chemical properties and molecular structure through the breaking and forming of bonds, requiring the absorption or release of energy. Reactions can be classified as endothermic or exothermic depending on how the system interacts with energy - endothermic reactions absorb heat from surroundings while exothermic reactions release heat, with endothermic reactants having lower energy than products and exothermic reactants having higher energy.
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This document provides an overview of thermodynamics, including definitions of key terms, types of systems and processes, the three laws of thermodynamics, and concepts like state functions, equilibrium, and exergonic and endergonic reactions. It defines thermodynamics as the branch of science dealing with different forms of energy and quantitative relationships between them. The objectives are to define terms, state the laws of thermodynamics and their limitations, explain applications to chemical reactions, and derive equations.
06 A Metabolism Energy Life Campbell
1. The document discusses metabolism and energy transformations in living organisms. It covers topics like metabolic pathways, ATP, the laws of thermodynamics, free energy, and exergonic and endergonic reactions.
2. Key points include that metabolic pathways convert energy from one form to another through chemical reactions, and that cellular respiration and photosynthesis involve exergonic and endergonic reactions, respectively.
3. The first and second laws of thermodynamics state that energy cannot be created or destroyed, and that entropy increases over time as energy is transferred or transformed.
Redoxtherm
Oxidation-reduction reactions are an important type of reaction in biochemistry that involve the transfer of electrons. Oxidation involves the loss of electrons and reduction involves the gain of electrons. These two processes must occur simultaneously. Thermodynamics is the study of energy and is important for understanding biochemistry. The first law of thermodynamics states that energy is conserved, while the second law states that spontaneous reactions result in an increase in the randomness or entropy of the universe. For a reaction to be spontaneous, the change in entropy of the universe must be positive.
Chapter 18
The common ion effect occurs when a salt with a common ion is added to a saturated solution of another salt containing that ion. This causes the solubility equilibrium of the original salt to shift left, decreasing the solubility.
When a common ion is added, the concentration of that ion increases on the product side of the solubility equilibrium expression. According to Le Chatelier's principle, this shift in concentration causes the equilibrium to shift left to counteract the change and re-establish equilibrium. Shifting left means more solid salt precipitates out of solution, decreasing the solubility.
So in summary, adding a common ion decreases the solubility of the original salt by shifting its solubility equilibrium left through the common ion effect.
Chapter 18
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.
An introduction to metabolism
This document provides an overview of metabolism and oxidative phosphorylation. It defines oxidative phosphorylation as the formation of ATP using energy released by electron transfer through electron carriers in the mitochondrial inner membrane. A proton gradient couples ATP formation to electron transfer. Catabolic pathways break down molecules and release energy, while anabolic pathways use energy to build molecules. ATP powers cellular work by coupling exergonic reactions that release energy to endergonic reactions that require energy. Enzymes lower the activation energy of reactions and increase their rates.
Thermo part 1
The document discusses the law of conservation of energy and thermo chemistry concepts. It defines a system and environment, and describes three types of systems: open, closed, and isolated. It explains that exothermic reactions release heat from the system while endothermic reactions absorb heat from the surroundings. The enthalpy change (ΔH) of a reaction is determined by subtracting the enthalpy of reactants from the enthalpy of products.
Energy Changes
Thermochemistry is the study of heat changes in chemical reactions. Energy is absorbed or released when bonds are broken and formed in a reaction. An exothermic reaction releases heat to the surroundings, while an endothermic reaction absorbs heat from the surroundings. The enthalpy change of a reaction indicates whether it is exothermic or endothermic.
1. Essentials of thermodynamics-1.pptx BSN
This document discusses key concepts in thermodynamics and their applications in biophysics. It introduces biophysics as applying physics principles to biological systems. Thermodynamics provides a framework to understand energy transformations in living organisms. The three laws of thermodynamics - zeroth law regarding thermal equilibrium, first law of energy conservation, and second law of entropy increase - are explained. The third law is also introduced. Examples are given of how these laws apply to biological processes like cellular respiration, protein folding, and temperature regulation. Biological thermodynamics is defined as studying biochemical dynamics controlled by energy processes like ATP hydrolysis and enzyme kinetics.
Thermo#2
This document defines different types of systems and their interactions with surroundings in thermodynamics. An open system can exchange both matter and energy with surroundings, a closed system can only exchange energy, and an isolated system cannot exchange either. Exothermic processes release heat to surroundings while endothermic processes absorb heat from surroundings. Vaporization and melting of substances are endothermic since they require energy, while freezing is exothermic as it releases energy.
Thermo#2
This document defines different types of systems and their interactions with surroundings in thermodynamics. An open system can exchange both matter and energy with surroundings, a closed system can only exchange energy, and an isolated system cannot exchange either. Exothermic processes release heat to surroundings while endothermic processes absorb heat from surroundings. Specific examples of endothermic processes that require energy input include vaporization and melting, while freezing is exothermic and releases energy.
5294953.ppt
Exothermic and endothermic reactions are differentiated based on whether heat is released or absorbed during the reaction. In exothermic reactions, more energy is released from the breaking and forming of bonds than is absorbed, resulting in a negative enthalpy change. These reactions release heat to the surroundings. In endothermic reactions, more energy is absorbed in bond breaking than released in bond forming, leading to a positive enthalpy change. Heat must be supplied from the surroundings for these reactions to proceed. Common examples of exothermic reactions include burning fossil fuels, while photosynthesis and melting substances are endothermic reactions that require energy input.
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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- 3. A chemical reaction involves not only changes in chemical properties but also in the structure of the substance. Change in structure involves either bond breakage or bond formation.When this happens energy is either released or absorved for the reaction to proceed.
- 4. Chemical reaction can also be classified as exothermic depending how the system interacts with energy. Endothermic reaction involves the absorption of heat by the system from the surroundings while exothermic reaction involves the release of heat by the system to the surroundings. Heat is referred to as the energy in transit from a body of higher gradient to a body of lower gradient.
- 5. Endothermic Reaction In an endothermic reaction,the system must absorb energy from from its surrounthings for the reaction to proceed.Thus ,the reactant has lower energy as compared with the product.
- 7. EXOTHERMIC REACTION On the other hand, for an exothermic reaction to happen,the system must release energy to the surroundings to attain stability of its product.Thus,the reactant has higher energy than its product