मराठी
महाराष्ट्र राज्य शिक्षण मंडळएचएससी विज्ञान (सामान्य) इयत्ता १२ वी

Rate constant of a reaction is 3.6 × 10–3 s–1. The order of reaction is ______.

Advertisements
Advertisements

प्रश्न

Rate constant of a reaction is 3.6 × 10–3 s–1. The order of reaction is ______.

पर्याय

  • first

  • second

  • third

  • zero

MCQ
रिकाम्या जागा भरा
Advertisements

उत्तर

Rate constant of a reaction is 3.6 × 10–3 s–1. The order of reaction is first.

shaalaa.com
  या प्रश्नात किंवा उत्तरात काही त्रुटी आहे का?
पाठ 6: Chemical Kinetics - Multiple choice questions

संबंधित प्रश्‍न

How will you represent first order reactions graphically.


Answer the following in brief.

Derive the integrated rate law for the first-order reaction,

\[\ce{A_{(g)} -> B_{(g)} + C_{(g)}}\] in terms of pressure.


Solve

The half-life of a first-order reaction is 1.7 hours. How long will it take for 20% of the reactant to react?


Time required for 100% completion of a zero order reaction is _______.


Give one example of a pseudo first-order reaction.


Write order of the following reaction:

\[\ce{2NH_{3(g)} -> N_{2(g)} + 3H_{2(g)}}\]


What is half life of first order reaction if time required to decrease concentration of reactants from 0.8 M to 0.2 M is 12 hours?


For the reaction 2NOBr → 2NO2 + Br2, the rate law is rate = k[NOBr]2. If the rate of a reaction is 6.5 × 10–6 mol L–1 s–1, when the concentration of NOBr is 2 × 10–3 mol L–1. What would be the rate constant of the reaction?


The rate constant of the first order reaction is 1.386 min–1. Calculate the time required for 80% reactant to decompose?


Write units of rate constants for:

  1. First-order reaction
  2. Zero-order reaction

This reaction follows first-order kinetics. The rate constant at particular temperature is 2.303 × 10−2 hour−1. The initial concentration of cyclopropane is 0.25 M. What will be the concentration of cyclopropane after 1806 minutes? (log 2 = 0.3010)


In a first order reaction \[\ce{x -> y}\]; if k is the rate constant and the initial concentration of the reactant x is 0.1 M, then, the half life is


The rate constant of a reaction is 5.8 × 10−2 s−1. The order of the reaction is ____________.


If 75% of a first order reaction was completed in 60 minutes, 50% of the same reaction under the same conditions would be completed in ____________.


A first order reaction is 40% complete in 50 minutes. Calculate the value of the rate constant. In what time will the reaction be 80% complete?


A first order reaction has a rate constant 0.00813 min-1. How long will it take for 60% completion?


For first order reaction the concentration of reactant decreases from 0.2 to 0.1 M in 100 minutes. What is the rate constant of the reaction?


If [A] is the concentration of A at any time t and [A]0 is the concentration at t = 0, then for the 1st order reaction, the rate equation can be written as ____________.


The rate and the rate constants of the reaction, \[\ce{A + 2B -> C + D}\] are 8 × 10−3 mol dm−3 s−1 and 2 × 10−3 s−1 respectively. The concentrations of A and B are 4 mol dm−3 each. The overall order of the reaction is ____________.


The time taken for 80% of a first order reaction to be complete is approximately ____________.


The rate of formation of B at time t for reaction \[\ce{2A -> 3B}\] is equal to ____________.


A first order reaction takes 40 minutes for 30% decomposition. What is the half-life of reaction?


In a reaction \[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\], if the rate of disappearance of N2(g) is 2.6 × 10−4 M/s, the rate of disappearance of H2(g) in M/s is ____________.


A first order reaction takes 40 minutes for 30% completion. Calculate the half-life of reaction.


Half-life of first-order reaction \[\ce{X -> Y + Z}\] is 3 minutes. What is the time required to reduce the concentration of 'X' by 90 % of it's initial concentration?


Which of the following reactions is not of the first order?


Which is the relation between half life and rate constant for a zero order?


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×