हिंदी

The time required for 90% completion of a certain first-order reaction is t. The time required for 99.9% completion will be _________.

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प्रश्न

The time required for 90% completion of a certain first-order reaction is t. The time required for 99.9% completion will be _________.

विकल्प

  • t

  • 2t

  • `"t"/2`

  • 3t

MCQ
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उत्तर

The time required for 90% completion of a certain first-order reaction is t. The time required for 99.9% completion will be 3t.

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अध्याय 6: Chemical Kinetics - Exercises [पृष्ठ १३५]

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बालभारती Chemistry [English] Standard 12 Maharashtra State Board
अध्याय 6 Chemical Kinetics
Exercises | Q 1. iv. | पृष्ठ १३५

संबंधित प्रश्न

Choose the most correct option.

The rate constant for the reaction \[\ce{2N2O5_{(g)} -> 2N2O4_{(g)} + O2_{(g)}}\] is `4.98 xx 10^-4 "s"^-1`. The order of reaction is _____________.


Choose the most correct option.

Slope of the graph ln[A]t versus t for first-order reaction is _________.


Answer the following in one or two sentences.

For the reaction, \[\ce{CH3Br_{(aq)} + OH^{-}_{(aq)} -> CH3OH^{\ominus}_{(aq)} + Br^{\ominus}_{(aq)}}\], rate law is rate = \[\ce{k[CH3Br][OH^\ominus]}\]

How does reaction rate changes if \[\ce{[OH^\ominus]}\] is decreased by a factor of 5?


Answer the following in one or two sentences.

For the reaction,

\[\ce{CH3Br_{(aq)} + OH^-_{ (aq)} -> CH3OH^-_{ (aq)} + Br^-_{ (aq)}}\], rate law is rate = k`["CH"_3"Br"]["OH"^-]`

What is the change in rate if concentrations of both reactants are doubled?


A First order reaction is 50% complete in 69.3 minutes. Time required for 90% completion for the same reaction is _______.


The rate law relates to the rate of a chemical reaction in terms of _______.


Order of reaction for which unit of rate constant is mol dm–3 s–1 is _______.


For the reaction \[\ce{2NO_{(g)} + 2H_{2(g)} -> N_{2(g)} + 2H2O_{(g)}}\],

The rate law is, rate = k[NO]2 [H2].

What is the overall order of reaction?


A reaction occurs in the following steps:

Step 1: \[\ce{NO_{2(g)} + F_2 -> NO2F_{(g)} + F_{(g)}}\] (slow)

Step 2: \[\ce{F_{(g)} + NO_{2(g)} -> NO_2F}\] (Fast)

  1. Write the equation of overall reaction.
  2. Write the rate law.
  3. Identify reaction intermediate.

For the reaction 2A + B → C, rate of disappearance of A 0.076 mol s –1.

  1. What is the rate of formation of C?
  2. What is the rate of consumption of B?
  3. What is the rate of the overall reaction?

In a hypothetical reaction,

\[\ce{2A + B -> Products}\]. Rate = k [A]2 [B]

Molar concentration of 'B' is kept constant and molar concentration of 'A' is tripled, then the rate of reaction will ____________.


The rate constant of a first order reaction whose half-life is 480 seconds, is ____________.


For the non-stoichiometric reaction

\[\ce{2A + B -> C + D}\], the following kinetic data were obtained in three separate experiments, all at 298 K.

Initial concentration
(A)
Initial concentration
(B)
Initial rate of formation of C
(mol dm−3 s−1)
0.1 M 0.1 M 1.2 × 10−3
0.1 M 0.2 M 1.2 × 10−3
0.2 M 0.1 M 2.4 × 10−3

The rate law for the formation of C is:


For the reaction, \[\ce{N2(g) + 3H2(g) -> 2NH3(g); \Delta H}\] is equal to ______.


A gaseous hypothetical chemical equation \[\ce{2A ⇌ 4B + C}\] is carried out in a closed vessel. The concentration of B is found to increase by 5 × 10−3 mol dm−3 in 10 second. The rate of ____________.


For a hypothetical reaction \[\ce{A + B -> C}\], it is found that doubling the concentration of A increases the rate by 8 times and doubling the concentration of B increases the rate by 4 times. The overall order of the reaction is ____________.


Select the rate law that corresponds to the data shown for the following reaction:

\[\ce{A + B -> C}\]

Exp. [A]
mol dm−3
[B]
mol dm−3
Initial Rate
mol dm−3
1. 0.012 0.035 0.10
2. 0.024 0.070 0.80
3. 0.024 0.035 0.10
4. 0.012 0.070 0.80

The rate law for the reaction \[\ce{A + B + C -> Product}\] is expressed as Rate = k[A]2 [B]1 [C]0. What is the overall order of the reaction?


The rate law for the reaction \[\ce{2NO_{(g)} + O2_{(g)} -> 2NO2_{(g)}}\] is rate = k[NO]2 [O2] , then which among the following statement is correct?


What is the order of reaction for decomposition of gaseous acetaldehyde?


What is the molecularity and order of the following reaction if rate law is, rate = k[O3][O] respectively.

\[\ce{O_{3(g)} + O_{(g)} -> 2O_{2(g)}}\]


For the reaction \[\ce{2A + B -> 3C + D}\], which among the following is NOT the correct rate law expression?


For the reaction \[\ce{4NH3 + 5O2 -> 4NO + 6H2O}\], the rate of disappearance of NH3 is 3.6 × 10-3 M/s. What is the rate of formation of water?


The correct order of raaii of F, F-, O and O2- is ______.


Write the rate law for the following reaction:

A reaction that is second order in NO and first order in Br2.


The rate constant of a reaction ______.


The rate constant for the reaction,

2N2O5(g) → 2N2O4(g) + O2(g) is 4.98 × 10-4 s-1.

What is the order of reaction?


`t_(1/4)` can be taken as the time taken for the concentration of a reactant to drop to `3/4` of its initial value. If the rate constant for a first order reaction is k, the `t_(1/4)` can be written as ______.


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