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{:("7. slow step","a. experimentally"),(...

`{:("7. slow step","a. experimentally"),("8. order","b. zero order"),("9. molecularity","c. rate determining step"),("10. unit of order 'k'","d. maximum rate"),("11. rate independent of reactant","theoretical concept concentration"),(,"f. "sec^(-1)):}`

Answer

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Starting from the rate law of a first order reaction, show that the half-life of the reaction is independent of the initial reactant concentration.

Write units of rate constant for zero order and for the second order reactions if the concentration is expressed in "mol.L"^(-1) and time in second.

Knowledge Check

  • Assertion (A) : The order and molecularity of the reaction is the same. Reason (R) : Order is determined experimentally. Molecularity is the sum of all the stoichiometric coefficients of the rate- determining elementary step.

    A
    (A) and (R) both are correct statements and (R) is correct explanation for (A).
    B
    (A) and (R) both are correct statements and (R) is not correct explanation for (A).
    C
    (A) is correct statement but (R) is wrong statement.
    D
    (A) is wrong statement but (R) is correct statement .

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    Determine the order of the following reactions : A reaction whose rate doubles on doubling the concentration of reactant .

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    The rate constant of a first order reaction is 0.0051"min"^(-1) . If the initial concentration of the reactant is 0.2(M) , find the concentration of the reactant after 2h.

    For the reaction A+2BrarrC+D , the rate of the reaction= k[A][B]^(2) where k = rate rate constant. How can the reaction be converted to a pseudo second order reactions?

    The rate constant of a reaction is 1.8xx10^3 min^(-1) . What is the order of the reaction?

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    The rate constant for a first order reaction is 60s^(-1) How much time will it take to reduce the initial concentration of the reactant to its (1)/(10) th value?

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