...Types of Chemical Reactions The vast number of chemical reactions can be classified in any number of ways. Under one scheme they can be categorized either as oxidation-reduction (electron transfer) reactions or non-oxidation-reduction reactions. Another completely different but common classification scheme recognizes four major reaction types: (1) combination or synthesis reactions (2) decomposition reactions (3) substitution or single replacement reactions (4) metathesis or double displacement reactions The Four Major Types of Reactions Name General Reaction Pattern Combination or synthesis A + B ----> AB Decomposition AB ----> A + B Substitution or Single Replacement A + BC ----> B + AC Metathesis or Double Displacement AB + CD ----> AD + CB Combination or Synthesis Reactions Two or more reactants unite to form a single product. S + O2 ---------> SO2 sulphur oxygen sulphur dioxide 2 S + 3 O2 ---------> 2 SO3 sulphur oxygen sulphur trioxide 2 Fe + O2 ---------> 2 FeO iron oxygen ...
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...CHEMICAL CONVERSIONS Acylation Acylation (rarely, but more formally: alkanoylation) is the process of adding an acyl group to a compound. The compound providing the acyl group is called the acylating agent. These are used to form aryl ketones. Because they form a strong electrophile when treated with some metal catalysts, acyl halides are commonly used as acylating agents. For example, Friedel-Crafts acylation uses acetyl chloride (ethanoyl chloride), CH3COCl, as the agent and aluminum chloride (AlCl 3) as a catalyst to add an ethanoyl(acetyl) group to benzene: The mechanism of this reaction is electrophilic substitution. Hydrolysis While solvolysis often refers to an organic chemistry context, hydrolysis is very common in inorganic chemistry, where aqua complexes of metal ions react with solvent molecules due to the Lewis acidity of the metal center. For example, aqueous solutions of aluminium chloride are acidic due to the aqua-aluminium complex losing protons to water molecules, giving hydronium ions which lowers the pH. In organic chemistry, hydrolysis reactions often give two fragments from an initial substrate. For example, the hydrolysis of amides give carboxylic acids and amines; the hydrolysis of esters give alcohols and carboxylic acids. Alcoholysis An example of a solvolysis reaction is the reaction of a triglyceride with a simple alcohol such as methanol or ethanol to give the methyl or ethyl esters of the fatty acid, as well as glycerol. This reaction is...
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...POINT LISAS CAMPUS Esperanza Road, Brechin Castle, Couva www.utt.edu.tt LAB 1 Decomposition reaction Aim: Determination of the number of moles of water molecules of crystallization present in hydrated Magnesium Sulphate (MgSO4.xH2O) Apparatus: Mass balance, test tube, test tube holder, heat-proof mat and bunsen burner. Reagents: Hydrated sodium carbonate. Theory: Chemical decomposition, analysis or breakdown is the separation of a chemical compound into elements or simple compounds. A more specific type of decomposition is thermal decomposition or thermolysis, which is caused by heat. ABA+B, the reaction is endothermic, since heat is required to break the chemical bonds. Most decomposition reaction require energy either in the form of heat, light or electricity. Absorption of energy causes the breaking of the bonds present in the reacting substance which decomposes to give the product. When a hydrated salt is heated it decomposes into a pure form of the salt and water. MgSO4.xH2O MgSO4 + H2O Procedure: Refer to Handout Results: A. Mass of test tube/g = 21.77 B. Mass of the tube and salt/g = 24.0 A table showing the mass of the test tube and salt after 3 consecutive heating: Heating | Mass of the test tube and salt/g | 1st | 23.96 | 2nd | 23.81 | 3rd | 23.81 | Calculations: G. Mass of anhydrous magnesium sulphate/g = F - A = 23.81 – 21.77= 2.04 H. Mass of water of crystallization evaporated/g...
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...Magnesium is an extremely reactive metal. When stored, it reacts with oxygen to form a layer of magnesium oxide on its surface. This layer of magnesium oxide is quite stable and prevents further reaction of magnesium with oxygen. The magnesium ribbon is cleaned by sand paper for removing this layer so that the underlying metal can be exposed to air. Question 2: Write the balanced equation for the following chemical reactions. (i) Hydrogen + Chlorine → Hydrogen chloride (ii) Barium chloride + Aluminium sulphate → Barium sulphate + Aluminium chloride (iii) Sodium + Water → Sodium hydroxide + Hydrogen Answer : (i) (ii) (iii) Question 3: Write a balanced chemical equation with state symbols for the following reactions. (i) Solutions of barium chloride and sodium sulphate in water react to give insoluble barium sulphate and the solution of sodium chloride. (ii) Sodium hydroxide solution (in water) reacts with hydrochloric acid solution (in water) to produce sodium chloride solution and water. Answer : (i) (ii) Question 1: A solution of a substance ‘X’ is used for white washing. (i) Name the substance ‘X’ and write its formula. (ii) Write the reaction of the substance ‘X’ named in (i) above with water. Answer : (i) The substance ‘X’ is calcium oxide. Its chemical formula is CaO. (ii) Calcium oxide reacts vigorously with water to form calcium hydroxide (slaked lime). Question 2: Why is the amount of gas collected in one of the test tubes in Activity 1...
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...Christian Rodriguez Mrs. Gentry AP Biology September 27, 2015 Lab Abstract Enzymes are proteins produced by living cells. In an enzyme, the substrates bind with the active site of an enzyme, breaking them down into other molecules. Enzymes acts as catalyst which lower the reaction energy and allows it to take place in less time and at lower temperatures. Enzymes can be used in a reaction without actually being used up; therefore, they can be used reversibly. Temperature, salt concentration, substrate concentration, enzyme concentration, and pH can affect enzyme reactions. If the pH is too basic, the enzyme gains (H+) and denaturalizes; likewise if the pH is too acidic, then the enzyme loses (H+) and becomes denaturalized. A major benefit...
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...Chemical Reactions Types of Chemical reactions Lots of reactions take place around us in everyday life. Reactions are quit important in chemistry and in science generally. Chemical reaction is the changing of substances to other substances by the breaking of bonds in reactants and the formation of new bonds in products. There are different types of chemical reaction: 1. Combination reaction 2. Decomposition reaction 3. Single-replacement reaction 4. Double-replacement reaction 5. Combustion reaction Combination reaction is a chemical change in which two or more substances to form a new single substance. The reactants of most common combination reactions are either two elements or two compounds. The product a combination reaction is always a compound. Decomposition reaction is a chemical change in which one substance is broken down into two or more products. These products can be any combination of elements and compounds. It is usually very difficult to predict the products of decomposition reactions. Single-replacement reaction is a chemical change in which the atoms of less active element are replaced with atoms of elements which are more active. Usually the reactants are substance and element. Whenever one metal will replace another metal from a compound can be determined by the relative activities of the two metals. For predicting the products of this type of reaction we have the metal activity table, which is expressed above. Li K Ca Na Mg Al ...
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...We recently did two labs where we were given the task of observing single-replacement and double-replacement reactions. This paper has background information on the different types of chemical reactions, as well as the chemistry behind the two reactions we observed in lab. A chemical reaction is a process that is characterized by a chemical change in which the reactants (starting products) are different from the products. Chemical reactions involve the breaking of old bonds and the formation of new bonds. They can result in the formation of precipitates, changes in color, production or absorption of heat, or formation of gas bubbles. Chemical reactions can be placed in the following five categories: (i) synthesis (ii) decomposition...
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...CHEMISTRY 1. CHEMICAL SUBSTANCES Students should be able to: (a) Define the following terms: o Element o Mixture o Compound o Symbol o Formulae o Atom o Molecule (b) Distinguish between elements, mixtures and compounds and give examples of each; (c) Recall that some metals are reactive and others are not; (d) Demonstrate an understanding of the reactivity series; (e) Arrange metals in order of reactivity (Sodium, Calcium, Magnesium, Zinc, Iron, Copper, Silver and Gold); (f) Recall what are acids and bases; (g) State the importance of acids and bases; (h) Recall the colours of indicators (methyl orange, phenolphthalein, litmus) in acids and alkalis 2. THE LANGUAGE OF CHEMISTRY Students should be able to: (a) Describe physical changes giving examples; (b) Describe chemical changes giving examples; (c) Give the symbols and valencies of elements; (d) Work out the formulae of compounds; (e) Define the term radical and give the names and valencies of the following radicals: hydroxide, carbonate, sulfate, ammonium and nitrate; (f) Demonstrate an understanding of chemical reactions, reactants and products; (g) Represent chemical reactions by word equations; (h) Convert word equations to balanced chemical equations; (i) Write and balance chemical equations 3. CHEMICAL REACTIONS IN GENERAL Students should be able to: (a) Describe the reaction of selected metals (sodium, magnesium, iron and copper)with oxygen; (b) Describe...
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...gas by using Hess’s law. Introduction: A reaction that release heat to surrounding is known as exothermic reaction. It is usually observed as temperature increases in solvent, container and other immediate surroundings. The expression of heat released from the reaction is: qreaction = qsolution + qcalorimeter ……..(1) The qcalorimeter is nearly zero because the calorimeter in this experiment is assumed to absorb little heat. So, the equation is simplified to qreaction = qsolution ……...(2) The change in temperature that caused by the addition of a given amount of heat will depend on specific heat, Csp of substance. Therefore, the heat involved is calculated by the equation Q = (Csp)(m)(T) ………(3) Mass of substance is m, change is temperature is T (final temperature – initial temperature). The heat changes observed is equal to enthalpies of reaction, H for the reactions considered because this experiment was run at constant pressure. The enthalpy of these directly observed reactions and Hess’s law was used to calculate the enthalpy change for an additional reaction which is not directly observed. Hess’s law stated that the overall enthalpy change of a chemical reaction is independent of its pathway. The magnitude of enthalpy change of a chemical reaction depends only on the difference in the enthalpy content of the products and the reactants, and does not depend on how the reaction is completed. Consider the below thermochemical...
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...My science fair project is based on a chemical reaction taking place to turn a hot substance into ice. A chemical reaction is a reaction that changes the substances original identity to a different chemical identity. There are many different types chemical reactions in chemistry, but the one we are going to be focusing on are exothermic reactions. Exothermic reactions are reactions that transfer energy to the surroundings. The exothermic reaction is a reaction that gives off more energy than it needs to in order to complete its reaction. The exothermic reaction in this project is between baking soda and vinegar. Baking soda is a bicarbonate and vinegar is a acetic acid. Baking soda is made up of 1 sodium, 1 hydrogen, 1carbon, and 3 oxygen atoms. Vinegar is composed of 2 carbon, 4 hydrogen, and 2 oxygen atoms. Baking soda is an alkaline object that is alike to some salt and it reacts to acidic substances. When baking soda reacts it gives off some type of gas, carbon dioxide. Baking soda is usually seen in cooking, cleaning substances around the house, and in may science projects due to its ability to react with acids. Baking soda is usually used to...
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...given out. (a) Name the iron salt (b) Name the type of reaction that takes place during the heating of iron salt. (c) Write a chemical equation of the reaction involved. 2. A strip of metal X is dipped in a blue coloured salt solution YSO4. After some time, a layer of metal Y from the salt solution is formed on the surface of metal strip X. Metal X is used in galvanisation whereas metal Y is used in making electric wires. Metal X and Y together form an alloy Z. (a) What could metal X be? (b) What could metal Y be? (c) Name the metal salt YSO4. (d) What type of chemical reaction takes place when metal X reacts with salt solution YSO4? Write the equation of the chemical reaction involved? (e) Name the alloy Z. 3. Consider the following equation of the chemical reaction of a metal M : 4M + 3O2----------------- 2M2O3 This equation represents: (a) Combination reaction as well as reduction reaction (b) Decomposition reaction as well as oxidation reaction (c) Oxidation reaction as well as displacement reaction (d) Combination reaction as well as oxidation reaction 4. Consider the reaction KBr(aq) + AgNO3 (aq) -------------- KNO3 (aq) + AgBr (s) This is an example of (a) Decomposition (b) Combination (c) Double displacement (d) Displacement reaction 5. Express the following facts in the form of chemical equation: “When a strip of copper metal is placed in a solution...
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...grams)(6.022x10^23)(Number of atoms/1molecule) * Molar mass - Molar mass is the weight of one mole (or 6.022 x 1023 molecules) of any chemical compounds. * Mass % of an element in a compound: * ((Number of atoms of element)(atomic weight))/(Formula weight) * Empirical formula – Gives the lowest whole number ratio of atoms of each element in a compound (Grams)/(atomic weight) --- divide by lowest number on all * Molecular formula – gives actual whole number ratio of atoms of each element in each compound. (Molecular formula weight)/(Empirical formula weight) x compound * Formulas from analysis: * Structured formula – a formula that shows the atoms of a compound, their relative positions, and the bonds between them. * Isomers – compounds with the same molecular formula, but different properties and different arrangements of atoms * Writing chemical equations (symbols) : * + adding 2 or more chemicals together * -> Yields (Products) * (arrow forward and backward) reaction in both directions (denotes equilibrium) * (arrow up) gas evolved * (arrow down) solid precipitate forms * (s), (l), (g) solid, liquid, gas * (aq) aqueous solution * (Triangle) heating the solution * Limiting reagent – the reagent that is completely consumed in a reaction * Reagent that limits the amount of product possible * Theoretical...
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...Carmel Vijay Chemistry Lab 227 Zach Sailor November 8, 2013 Observing Chemical Reactions Beginning Question When a chemical reaction takes place, is it always accompanied by a physical change? Explain. Bunsen burner The Bunsen burner is a device in use these days to safely burn a continuous stream of a flammable gas such as natural gas, propane, or butane. The completeness of the combustion reaction affects the amount of air mixed with the gas stream. When a gas stream is well mixed with air, it provides oxygen in an equimolar amount which results in a complete and hotter reaction. We learned how to control the amount of air that is provided for the appearance of a blue flame, which is considered the right flame for a reaction. The evidence that led me to this conclusion was a few articles that explained that the yellow flame or also known as the “dirty flame” leaves behind a layer of carbon on whatever it is heating. Also when tested on a piece of copper wire, it took a longer time for a reaction to occur, whereas the blue flame created a faster reaction which stripped the copper coating off the wire. Chemical reaction The chemical reactions that were chosen, were chose based on which reaction is a more “green” reaction. A1: place a pea-sized amount if baking soda NaHCO3 in a test tube. Add 10-20 drops of vinegar drop wise. B2: place approx. 1Ml of 0.1M of MgCl2 in a test tube. Add an equal volume of NaOH drop wide. Stir well. C1: drop a pea-sized wad of...
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...I Intro In this lab we are going to observe chemical reactions. A chemical reaction is the rearrangement of stuff into new stuff. When a chemical reaction occurs there is color change, temperature change, energy change, gas release, odor, and precipitation. There are 5 different types of chemical reactions: synthesis, decomposition, single displacement, double displacement, and combustion. A chemical reaction has to be balanced because of the law of conservation of mass. Conservation of mass is mass neither created nor destroyed. The product has to be the same amount of substances as the reactants. II Purpose The purpose of this lab is to observe different typed of chemical reactions. III Data / Observations Reaction #1: 2Mg + O2 2MgO Synthesis * Burning magnesium metal turns it into an ultraviolet light while on fire. Product is a white powder. Reaction #2: Mg + HCl MgCl2 + H2 Single displacement * When magnesium was added to HCl, it started to bubble and the test tube became hot. When a flame lit on a wooden splint was added it made a loud pop sound. Reaction #3: (NH4)2 + CO3 (NH4)2 + CO3 Decomposition * Ammonium carbonate was added into a test tube and heated up it up with fire. After adding a piece of litmus paper a strong odor was released. The litmus paper turned from a color pink to a color of blue. Reaction #4: CaCo3 + 2HCl CaCl2 + H2CO3 Double displacement * When HCl was added to calcium carbonate it began...
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...Purpose How do we determine the reaction type and write a balanced equation for chemical reactions? Background Discussion There are many kinds of chemical reactions and several ways of classifying them. One popular and useful method is to classify reactions into five major types. These are: (1) synthesis, (2) decomposition, (3) single replacement, (4) double replacement, and (5) combustion. Most reactions can be put into one of these categories. In a synthesis reaction, two or more substances (elements or compounds) combine to form a more complex substance. A decomposition reaction is exactly the opposite of a synthesis reaction. In a decomposition reaction, a compound breaks down into two or more simpler substances (elements or simpler compounds.) In a single replacement reaction, one element in a compound is replaced by a more active element. In a double replacement reaction, the positive ions of two different ionic compounds can be thought of as “replacing each other.” Most replacement reactions (both single and double) take place in aqueous solutions containing free ions. In a double replacement reaction, one of the products must be removed from the solution as a precipitate, water, or an insoluble gas. A precipitate is a solid that is produced as a result of a chemical reaction in solution. As the precipitate separates from the solution, the solution appears cloudy. In a combustion reaction a substance combines with oxygen, releasing a large amount...
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