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The integrated rate equations can be fit...

The integrated rate equations can be fitted with kinetic data to determine the order of a reaction. The integrated rate equations for zero, first and second order reactions are : Zero order : `[Al =-kt+ [A]_0` First order : `log [A] = -(kt)/2.303 + log [A]_0` Second order : `1/([A])=kt+1/[A]_0` These equations can also be used to calculate the halt life periods of different reactions, which give the time during which the concentration of a reactant is reduced to half of its initial concentration, i.e, at time `t_(1//2), [A] = [A]_0//2` Answer the following (1 to 5) question : For a second order reaction, rate at a particular time is x. if the initial concentration is tripled, the rate will become

A

`9 x^2`

B

27x

C

9x

D

3x

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The integrated rate equations can be fitted with kinetic data to determine the order of a reaction. The integrated rate equations for zero, first and second order reactions are : Zero order : [Al =-kt+ [A]_0 First order : log [A] = -(kt)/2.303 + log [A]_0 Second order : 1/([A])=kt+1/[A]_0 These equations can also be used to calculate the halt life periods of different reactions, which give the time during which the concentration of a reactant is reduced to half of its initial concentration, i.e, at time t_(1//2), [A] = [A]_0//2 Answer the following (1 to 5) question : For a second order reaction, the correct plot of t_(1//2) vs. 1//[A]_0 is

The integrated rate equations can be fitted with kinetic data to determine the order of a reaction. The integrated rate equations for zero, first and second order reactions are : Zero order : [Al =-kt+ [A]_0 First order : log [A] = -(kt)/2.303 + log [A]_0 Second order : 1/([A])=kt+1/[A]_0 These equations can also be used to calculate the halt life periods of different reactions, which give the time during which the concentration of a reactant is reduced to half of its initial concentration, i.e, at time t_(1//2), [A] = [A]_0//2 Answer the following (1 to 5) question : The rate for the first order reaction is 0.0069 mol L^-1 mi n^-1 and the initial concentration is 0.2 mol L^-1 . The half life period is

Knowledge Check

  • For Zero order reaction. The integrated rate equation is :

    A
    `kt = [A]//[A]_0`
    B
    `kt=[A] – [A]_0`
    C
    `[A] =- kt +[A] `
    D
    `[A] =kt -[A]_0`

  • Half life period of a zero order reaction is

    A
    `t_(1//2) = 0.693 k`
    B
    `t_(1//2) = [A]_0//2K`
    C
    `t_(1//2) = 1//k[A]_0`
    D
    none of the above.

  • Half life period of a first order reaction is :

    A
    directly proportional to the initial concentration of reactant
    B
    half of the rate constant
    C
    same for all reactions
    D
    independent of the initial concentration of the reactants

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    The integrated rate equations can be fitted with kinetic data to determine the order of a reaction. The integrated rate equations for zero, first and second order reactions are : Zero order : [Al =-kt+ [A]_0 First order : log [A] = -(kt)/2.303 + log [A]_0 Second order : 1/([A])=kt+1/[A]_0 These equations can also be used to calculate the halt life periods of different reactions, which give the time during which the concentration of a reactant is reduced to half of its initial concentration, i.e, at time t_(1//2), [A] = [A]_0//2 Answer the following (1 to 5) question : The decomposition of nitrogen pentoxide : 2N_2O_5(g) rarr 4NO_2(g) + O_2(g) is a first order reaction. The plot of log [N_2O_5] vs time (min) has slope = - 0.01389. The rate constant k is

    Define order of a reaction. Give the units of rate constant for first and second order reactions.

    Define zero order reaction. Derive integrated rate equation for rate constant of a zero order reaction.

    Order of a reaction can be zero.

    The half life period for a zero order reaction is equal to

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