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Rates of Reaction....!

Rates of Reaction....!. 02. What is meant by the term rates of reaction? What does rate refer too... What does reaction refer too So putting it together rates of reaction simply means how fast a reaction occurs. RATES OF REACTION.

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Rates of Reaction....!

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  1. Rates of Reaction....!

  2. 02 • What is meant by the term rates of reaction? • What does rate refer too... • What does reaction refer too • So putting it together rates of reaction simply means how fast a reaction occurs.

  3. RATES OF REACTION • The rate of a reaction can also refer to how quickly or slowly the reactants disappear and the products appear • So now we know what is the rate of a reaction, what is the principle behind it?

  4. Collision Theory • Lets look at this short animation and see what we get from it. • collision theory explained [www.keepvid.com].mp4

  5. Collision Theory • First we must understand what causes reactions to occur. In order for a reaction to occur molecules must collide with each other(collision theory). In collision particles must have.. • Correct orientation • Enough energy(activation energy)

  6. Factors Affecting Rate of Reaction • Now we know the principle behind a reaction let’s see what are the factors that can affect the rate of a reaction. • Lets try these activities and see what we can uncover about the factors that influence how fast or slow a reaction occurs

  7. 1.Concentration • Increasing the rate of reaction, increases the number of molecules present, hence increasing the chances of the number of collisions. The more collisions possible the greater the rate of reaction.

  8. 2.Temperature • Increasing the temperature increases the amount of energy the particles possess. The more energy a particle contains the more movement takes place. The greater the movement of particles the greater the chance of collision and hence an increase in rate of reaction.

  9. 3.Surface area • Increasing the surface area increases the area on which particles can collide. Again, increasing the amount of collision increase the rate of reaction

  10. 4.Catalyst • A catalyst is a substance that speeds up a reaction but is chemically unchanged at the end. It increases rate by decreasing the amount of energy required for a reaction to occur(activation energy). It can be seen as providing an alternative route for a reaction(like taking a shortcut).

  11. NOTE AN ENZYME IS A NATURAL CATALYST. THE ENZYMES PRESENT IN THE PROCESS OF DIGESTION HELP SPEED UP THE DIGESTION PROCESS.

  12. 5. Light • Light is a form of energy. The more energy present the greater the movement of particles hence the more collisions taking place. Increasing the collision then increases the rate of reaction

  13. 6.Pressure(for gaseous systems) • Increasing pressure decreases the volume bringing the particles closer together (volume is inversely proportional to pressure-Gas Laws). This increases the number of collision hence the rate of reaction increases

  14. HOW IS THE UNDERSTANDING OF RATES IMPORTANT TO US IN OUR EVERYDAY LIFE?

  15. RATES IN ACTIONsometimes we need to.. • SPEED UP REACTION • Manufacturers usually wish to increase the rate of reaction as much as possible to produce maximum product in minimum time at low cost • Digestion • SLOW DOWN REACTION • Food spoiling • Ripening of fruits • Rusting

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