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What is effective collision ?...

What is effective collision ?

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Effective collision is that due to which formation of products takes place and results in the chemical reaction. In this, breaking of old bonds of reactants and formation of new bonds of products take place.
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According to collision theory of chemical reactions, rate of a reaction depends upon collision frequency and fraction of effective collisions. The rate of a reaction generally increases with rise in temperature mainly because of increase in number of effective collisions. Arrhenius proposed a quantitative relation between rate constant and temperature as k= Ae^(-E_a//Rt) where E_a is activation energy. It is equal to the difference between threshold energy and average kinetic energy of reacting molecules. Which of the following plot will be linear ?

Knowledge Check

  • According to collision theory, rate of the reaction effects by which of the following: 1. reacting molecules must react in the presence of catalyst. 2. molecules must have energy equal to or high E_a 3. molecules must have effective collisions due to proper orientation. 4. none of these.

    A
    both 1 and 4
    B
    both 2 and 3
    C
    1, 2 and 3
    D
    1,2,3 and 4
  • Effective collisions are when

    A
    molecules have attained the threshold energy
    B
    the molecules are in proper orientation
    C
    products are formed
    D
    all the above.
  • The effective collisions between the reactant molecules at higher temperatures ________.

    A
    Increase
    B
    Decrease
    C
    Remains same
    D
    First increase then decrease
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