Chemical reaction by muhammad shakaib qureshi
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Transcript of Chemical reaction by muhammad shakaib qureshi
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CHEMICAL REACTIONSfor Class DAE 1st Year Chemical Technology
MUHAMMAD SHAKAIB QURESHI
M.PHIL CHEMISTRY
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CONTENT
• INTRODUCTION
• COLLISION THEORY OF MOLECULE
• TYPES OF CHEMICAL REACTIONS
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Introduction
• Chemical reaction, a process in which one or more substances, the reactants, are converted to one or more different substances, the products. Substances are either chemical Element or Compound.
• Reactants are in left Hand Side Which Reacts together and formed products which are in right hand Side.
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Combustion Reaction
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How Chemical Reaction Happens ?Collision Theory of Molecules
Postulates• In order for a chemical reaction to take place, the reactants
must collide. The collision between the molecules in a chemicalreaction provides the kinetic energy needed to break thenecessary bonds so that new bonds can be formed.
• Sometimes, even if there is a collision, not enough kineticenergy is available to be transferred — the molecules aren’tmoving fast enough. You can help the situation somewhat byheating the mixture of reactants. The temperature is ameasure of the average kinetic energy of the molecules;raising the temperature increases the kinetic energy availableto break bonds during collisions.
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Continue
• Sometimes, even if there is a collision, not enoughkinetic energy is available to be transferred — themolecules aren’t moving fast enough. You can helpthe situation somewhat by heating the mixture ofreactants. The temperature is a measure of theaverage kinetic energy of the molecules; raising thetemperature increases the kinetic energy available tobreak bonds during collisions.
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• The molecules must also collide in the right orientation, or hit at the rightspot, in order for the reaction to occur.
• Here’s an example: Suppose you have an equation showing molecule A-Breacting with C to form C-A and B, like this:
• A-B + C→C-A + B• The way this equation is written, the reaction requires that reactant C
collide with A-B on the A end of the molecule. If it hits the B end, nothingwill happen. The A end of this hypothetical molecule is called the reactivesite, the place on the molecule that the collision must take place in orderfor the reaction to occur.
• If C collides at the A end of the molecule, then there’s a chance thatenough energy can be transferred to break the A-B bond. After the A-Bbond is broken, the C-A bond can be formed. The equation for this reactionprocess can be shown in this way:
• C~A~B→C-A + B• So in order for this reaction to occur, there must be a collision between C
and A-B at the reactive site. The collision between C and A-B has to transferenough energy to break the A-B bond, allowing the C-A bond to form.
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Energy is required to break a bond between atoms.
ACTIVATION ENERGY
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Factors Affecting on Chemical Reaction
• Nature of Reactant
• Catalyst
• Concentration
• Temperature
• Pressure
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Example
Catalyzed Reaction
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Types of Chemical Reactions
• Addition/Synthesis Reactions:
• Addition reactions, also known as synthesis reactions or direct combination reactions, involve two or more reactants combining to form a single, more complex product. Examples are the reaction of iron and sulfur to form iron sulfide, or, in organic chemistry, the reaction of ethene and bromine to form dibromoethane.
• Example: C2H4 + Br2 → C2H4Br2
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• Decomposition Reactions:
• A decomposition reaction involves the breaking down of a chemical compound into elements or simpler compounds. It is sometimes defined as the opposite of a synthesis reaction. They can occur spontaneously, or be initiated by heat, a catalyst, or electrolysis. An example is the decomposition of hydrogen peroxide into hydrogen and oxygen.
• Example: 2H2O2 → 2H2O + O2
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• Combustion Reactions:
• Combustion reactions involve oxygen reacting with another element or compound to produce energy in the form of heat & light. They are always exothermic. Complete combustion requires a plentiful supply of oxygen – in a limited supply, incomplete combustion occurs, and different products can be formed. When organic chemicals combust completely, the products always include carbon dioxide and water.
• Example: CH4 + 2O2 → 2H2O + CO2
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• Neutralization Reactions:
• A neutralization reaction is one in which an acid and a base react to form a salt. Water is commonly produced as well. Often these reactions are exothermic, but endothermic neutralizations are possible. Neutralization reactions do not necessarily result in a pH of 7 – resultant pH is dependent on the strength of the acid and the base.
• Example: NaOH + HCl → NaCl + H2O
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• Precipitation Reactions:
• A precipitation reaction is one in which aqueous compounds react to form an insoluble solid, called a precipitate. This solid can be suspended throughout the solution, or fall to the bottom of the reaction vessel. Whether or not the product of a reaction will form a precipitate is determined by solubility rules for ionic compounds.
• Example: 2NaOH(aq) +MgCl2(aq) → 2NaCl(aq) + Mg(OH)2(s)
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• METATHESIS OR DOUBLE DISPLACEMENT REACTION
• In a double displacement or metathesis reaction two compounds exchange bonds or ions in order to form Different Compounds.
AB + CD → AD + CB
An example of a double displacement reaction occurs between sodium chlorideand silver nitrate to form sodium nitrate and silver chloride.
NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s)
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• SUMMARY
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THE END