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Chemical Kinetics Test - 3
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Chemical Kinetics Test - 3

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  • Question 1/10
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    For gaseous reaction, the rate can be expressed as

     

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  • Question 2/10
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    The initial rates of reaction for the equation, 2A + B →Products.

    Products were determined under various initial concentrations of reactants.

    Thus, rate law is equal to

     

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    Let order w.r.t. A = a, order w.r.t. B = b


     

     

  • Question 3/10
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    For the reaction, A + 2B →Product, the reaction rate was halved on doubling the concentration of A. Thus, order w.r.t. A is

     

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    If concentration of the nth order reaction is made m time, rate becomes mn times.


     

     

  • Question 4/10
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    Direction (Q. Nos. 14  and 15) This section contains a passage describing theory, experiments, data, etc. Two questions related to the paragraph have been given. Each question has only one correct answer out of the given 4 options (a), (b), (c) and (d)

    Passage  

    The decomposition of NO2 at 400 K proceeds at a of rate of 5.4 x 10-5 mol L-1 s-1 when [NO2 ] = 0.01 mol-1

    2 NO2 (g) →2NO(g ) + O2 (g).

    Q. What is the rate law when observed rate is 1.35 x 10-5  mol L-1  s-1   at [NO2 ] = 0.005 mol L-1 ?

     

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    Correct answer is option (D).
    The given information can be summarized as follows:

    Decomposition of NO2:
    - Reaction: 2 NO2(g) →2NO(g) + O2(g)
    - At 400 K: Rate = 5.4 x 10^(-5) mol L^(-1) s^(-1), [NO2] = 0.01 mol L^(-1)
    - Observed rate: 1.35 x 10^(-5) mol L^(-1) s^(-1), [NO2] = 0.005 mol L^(-1)

    Let 's compare the rates and concentrations given in the problem:

    Rate1 = 5.4 x 10^(-5) mol L^(-1) s^(-1), [NO2]1 = 0.01 mol L^(-1)
    Rate2 = 1.35 x 10^(-5) mol L^(-1) s^(-1), [NO2]2 = 0.005 mol L^(-1)

    Take the ratio of the two rates:

    Rate2/Rate1 = (1.35 x 10^(-5))/(5.4 x 10^(-5)) = 1/4

    Now, take the ratio of the two concentrations:

    [NO2]2/[NO2]1 = (0.005)/(0.01) = 1/2

    We can now evaluate each of the rate law options:

    a. k[NO2]: (1/2) ≠1/4
    b. k[NO2]^0: 1 ≠1/4
    c. k[NO2]^3: (1/2)^3 ≠1/4
    d. k[NO2]^2: (1/2)^2 = 1/4

    Only option (d) satisfies the relationship between the rates and concentrations:
    Rate Law:
    - k[NO2]^2

     

     

  • Question 5/10
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    The decomposition of NO2 at 400 K proceeds at a of rate of 5.4 x 10-5 mol L-1 s-1 when [NO2 ] = 0.01 mol-1

    2 NO2 (g) →2NO(g ) + O2 (g).

    Q. Rate constant of the reaction will be  

     

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  • Question 6/10
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    Direction (Q. Nos. 16-18) This section contains 3 questions. When worked out will result in one integer from 0 to 9 (both inclusive)

    In the following reaction

    Q. Where negative sign indicates rate of disappearance of the reactant. What is the value of x/y ?

     

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  • Question 7/10
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    The reaction rate is defined as the rate at which the concentration of the reactants __________ with time or the concentration of products ___________ with time.

     

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    The reaction rate is defined as the rate at which the concentration of the reactants decreases with time or the concentration of products increases with time.

     

     

  • Question 8/10
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    In a certain polluted atmosphere containing O3 at a steady concentration of 2.0 x 10-6 M, the hourly production of O3 by all sources was estimated as 7.2 x 10-15 M. If the only mechanism for destruction of O3 in the second-order reaction is

    2O3  →3O2

    then rate constant for destruction reaction, defined by the rate law for - Δ[O3 ]/Δf is x * 10-7 M-1 s-1 . What is the value of x?

     

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  • Question 9/10
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    Only One Option Correct Type

    This section contains 2  multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct

    For a reversible reaction, net rate is  

    hence given reaction is  

     

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    2A - B →(reversible) C

    For a forward reaction, (dx/dt)f = k1 [A]2 [B]-1
    For a backward reaction, (dx/dt)b = k2 [C]

    Net rate = (dx/dt)f - (dx/dt)b   = k1 [A]2 [B]-1 - k2 [C]

     

     

  • Question 10/10
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    Reaction kinetics deals with the study of

     

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    Reaction kinetics deals with the study of rate of reaction, their mechanism and the factors which affects the rate of reaction. It specifies all the general characteristics of a chemical reaction.

     

     

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