Bio catalysis based bio sensor seminor
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It is a bio sensor based presentation, this presentation done by Alagu devi dpt of Bioelectronics and Biosensors at Alagappa University
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This document provides an overview of chemical reactions and energetics for a 10th grade IGCSE course. It discusses exothermic and endothermic reactions in relation to energy changes and temperature. It also covers the factors that affect reaction rates, including concentration, particle size, catalysis, and temperature. The document defines oxidation and reduction in terms of electron transfer and identifies redox reactions. It provides examples of exothermic and endothermic reactions and discusses how catalysts can lower the activation energy and increase reaction rates. Interactive links are included to illustrate and reinforce the concepts.
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The document discusses different types of chemical reactions:
1) Decomposition reactions involve a single compound breaking down into simpler substances. An example is calcium carbonate decomposing to calcium oxide and carbon dioxide.
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3) Single replacement reactions involve an element replacing another in a compound. An example is copper displacing silver from silver nitrate.
4) Double replacement reactions involve ion exchange between two compounds in solution and forming a precipitate. An example is silver nitrate and sodium chloride forming silver chloride and sodium nitrate precipitates.
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1. The document discusses chemical reactions, including what makes something a chemical reaction, different ways to describe reactions using word equations, chemical equations, and balanced equations.
2. It describes the main types of chemical reactions - synthesis, decomposition, single replacement, double replacement, and combustion reactions - and provides examples of each.
3. Guidelines are given for writing balanced chemical equations, including identifying the reaction type and using coefficients to balance the mass on each side.
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Chemical reactions involve the transformation of one or more substances into different substances. There are two types of substances involved: reactants present at the beginning of the reaction and products formed by the reaction. Chemical reactions obey the law of conservation of mass, meaning the total mass of the reactants equals the total mass of the products. Evidence of a chemical reaction may include the absorption or release of energy, a change in color or odor, the formation of a gas, or the production of a precipitate. Chemical equations are used to represent chemical reactions, and must be balanced so the number of atoms of each element is the same on both sides of the reaction.
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3) Decomposition reactions involve complex molecules breaking down into simpler ones.
4) Single displacement reactions involve one element replacing another in a compound.
5) Double displacement reactions involve the switching of anions and cations between compounds to form new compounds.
6) Acid-base reactions specifically involve acids and bases reacting to form water and an ionic salt.
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This document discusses chemical reactions and equations. It defines a chemical reaction as a process where reactants are converted into products, which may occur under the influence of a catalyst. It describes how to write word and chemical equations, and how to balance chemical equations by ensuring equal numbers of each type of atom on both sides. It also defines and provides examples of different types of chemical reactions: combination, decomposition, displacement, double displacement, and redox reactions. Corrosion and rancidity are discussed as examples of oxidation reactions.
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1) Surface area - Increasing the surface area of a solid reactant increases the reaction rate by providing more collision sites.
2) Concentration - Increasing the concentration of a reactant increases the number of collisions between reacting particles and thus increases the reaction rate.
3) Temperature - Raising the temperature increases the kinetic energy of reacting particles, allowing more collisions with sufficient energy to result in reaction. This generally causes reaction rates to increase exponentially with temperature increases.
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The document discusses reversible reactions and the Haber process for producing ammonia from nitrogen and hydrogen. It notes that the Haber process uses high pressure of around 200 atmospheres, a temperature of 450°C, and an iron catalyst. At equilibrium, the reaction mixture is cooled to liquefy the ammonia, which is then separated from the recycled unreacted nitrogen and hydrogen for another cycle. The conditions aim to increase ammonia yield while maintaining a fast reaction rate and reasonable costs.
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Matter in our surroundings consists of particles that occupy space and have mass. Solids have a definite shape and volume, liquids have a fixed volume but no definite shape, and gases have neither a definite shape nor volume. The three states of matter - solid, liquid, and gas - differ in their compressibility, with gases being the most compressible and solids the least. A change of state, such as melting or boiling, requires an input of heat energy known as latent heat. The temperature and pressure at which melting, freezing, boiling, and condensation occur depend on the type of substance and can be used to characterize its properties.
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All chemical bonds contain potential energy that is changed during chemical reactions when old bonds break and new bonds form. There are several evidences that can indicate if a chemical reaction has occurred, including the emission of light, evolution of a gas, and changes in temperature, color, or the formation of a precipitate. Chemical equations are used to represent chemical reactions, and they must be balanced by ensuring equal numbers of each type of atom on both sides of the reaction.
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This chapter discusses chemical reactions and bonds. It explains that chemical bonds form when atoms exchange or share electrons, forming ionic bonds or covalent bonds. Chemical reactions involve reactants changing into products, and require activation energy to break existing bonds. Photosynthesis is highlighted as the key reaction that harnesses solar energy to produce glucose and oxygen, storing energy in chemical bonds and removing carbon dioxide from the atmosphere.
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1. A chemical reaction involves the formation of new substances through the rearrangement of atoms. Reactants undergo chemical changes to form products with different properties.
2. A chemical equation symbolically represents a chemical reaction, showing the reactants on the left and products on the right, separated by an arrow.
3. Key types of chemical reactions include combination, decomposition, displacement, and redox reactions. Combination reactions form one product from two or more reactants, while decomposition reactions involve a single reactant breaking into multiple products.
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water can be consider as a potentially green solvent.it is safest & least expensive solvent. organic reaction in aqueous medium.like deals alder reaction,pinacol coupling.
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- Chemical reactions involve reactants transforming into products through rearrangement of atoms.
- There are five main types of chemical reactions: combination, decomposition, single replacement, double replacement, and combustion.
- The type of reaction can be identified based on the reactants. Balancing chemical equations ensures the same number and type of atoms are on both sides.
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This document discusses reaction rates and chemical equilibrium. It begins by defining reaction rates and factors that influence reaction rates such as temperature, concentration, surface area, and catalysts. It then explains collision theory and the role of activation energy in reactions. The document also covers Le Chatelier's principle, how stresses such as concentration, temperature, and pressure affect chemical equilibrium. It defines equilibrium constants and discusses solubility equilibrium, including solubility product constants and the common ion effect. Finally, it introduces entropy, the role of entropy in spontaneous reactions, and free energy.
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This document provides an overview of simple chemical reactions, including:
1. It defines chemical reactions and gives examples of reactions that occur in everyday life like cooking and rusting.
2. It explains the difference between physical and chemical changes and identifies signs that a chemical reaction is occurring.
3. It describes reactants and products, explaining that reactants change into products in a chemical reaction.
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Bio catalysis based bio sensor seminor
- 2. A catalyst is a substance that increases the rate at which a chemical reaction approaches equilibrium, but is not consumed in the process. Catalyst affects only the rate of the reaction Most catalysts used in industrial and research laboratories are inorganic (often organometallic) compounds.
- 4. Catalysts can: • Make a reaction possible under achievable conditions • Reduce the necessity of expensive & dangerous conditions • Generate high yields and high product purity • Reduce the amount of side-product and waste created
- 5. Catalysts can be divided into two main types Catalysts Heterogeneous Homogeneous
- 6. This involves the use of a catalyst in a different phase from the reactants. Typical examples involve a solid catalyst with the reactants as either liquids or gases.
- 7. The hydrogenation of a carbon-carbon double bond The simplest example of this is the reaction between ethylene and hydrogen in the presence of a nickel catalyst.
- 8. Ethylene molecules are adsorbed on the surface of the nickel. The double bond between the carbon atoms breaks and the electrons are used to bond it to the nickel surface.
- 9. Hydrogen molecules are also adsorbed on to the surface of the nickel. When this happens, the hydrogen molecules are broken into atoms. These can move around on the surface of the nickel.
- 10. If a hydrogen atom diffuses close to one of the bonded carbons, the bond between the carbon and the nickel is replaced by one between the carbon and hydrogen.
- 11. That end of the original ethylene now breaks free of the surface, and eventually the same thing will happen at the other end.
- 12. As before, one of the hydrogen atoms forms a bond with the carbon, and that end also breaks free. There is now space on the surface of the nickel for new reactant molecules to go through the whole process again.
- 13. The proton is the most pervasive homogeneous catalyst because water is the most common solvent. Water forms protons by the process of self-ionization of water In an illustrative case, acids accelerate (catalyse) the hydrolysis of esters: CH3CO2CH3 + H2O CH3CO2H + CH3OH
- 14. Biocatalyst is a substance, for instance an enzyme or hormone, which initiates or increases the rate of a chemical reaction. A biocatalyst is also known as a biochemical catalyst. A biochemical catalyst normally an enzyme.
- 15. EXAMPLE OF AN ENZYME BIOSENSOR ◦ The most widespread biosensor today is the glucose biosensor. ◦ It is very often used to measure the glucose concentration in blood. ◦ There are quite a few enzymes which could be used as glucose detectors. ◦ The following example shows the glucose enzyme reaction with glucose oxidase.