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Energy of activation and orientation of...

Energy of activation and orientation of molecule together determine the criteria for effective collision . Explain.

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In the molecular collision theory of reaction rates ,
Rate constnat `K = Pze^(-E_(a)//RT)`
Here P is the orientation factor and Z is the collision factor .
The product of P and Z is the pre - exponential factor , A in the Arrhenius theory.
Rate constant `K = Ae^(-E_(a)//RT)`
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AAKASH SERIES-CHEMICAL KINETCS-EXERCISE - 3.2
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  2. Discuss on the kinetic spontaneity of a chemical reaction. Is a slow r...

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  3. Why the reactions involving covalent substances are slow? How they can...

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  4. How are rate and rate constant related to a free radical reaction?

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  5. Write on the concept of reaction rate with respect to reactant and wit...

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  6. What are reaction rate and specific rate? Write their units.

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  7. What is the role played by catalyst to alter the rate of reaction? Exp...

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  8. Time requires for 99% completion of a first order reaction is twice to...

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  9. Acid hydrolysis of ester is more rapid in heavy water than in water. W...

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  10. A collision that attains threshold energy level need not be successful...

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  11. Decomposition of ozone to oxygen proceeds in two steps : Setp 1 (fast...

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  12. A to products. The concentration of A changes from 0.2 to 0.15 mol L^...

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  13. Cl(2) + 2I^(-) to 2CI^(-) + I(2) , was carried out in water . Initia...

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  14. Bond energy and orientation play a role in the determination of effect...

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  15. What is activated complex? How is it formed and transformed into produ...

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  16. Discuss the energy barrier diagram for reaction rates. When the reacti...

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  17. The rate of a reaction triples when temperature changes from 20^(@)C t...

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  18. The rate constant at 0^(@)C is 7.87 xx 10^(-7)s^(-1) for a reaction wh...

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  19. Decomposition of X and Y obey first order with half lives 54 and 18 mi...

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  20. In the chemical reaction, 3A + B to 2C + 3D, the rate of appearance o...

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  21. Decay constant of a nuclear reaction is temperature independent. Why?

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