JEE Questions for Chemistry Chemical Kinetics Quiz 10 - MCQExams.com

Which of the following is the expression for Arrhenius equation ?

  • Chemistry-Chemical Kinetics-1807.png
  • 2)
    Chemistry-Chemical Kinetics-1808.png

  • Chemistry-Chemical Kinetics-1809.png
  • All the above
At 290 K velocity constant of a reaction was found to be 3.2 × 10-3 . At 300 K, it will be
  • 1.6 × 10-3
  • 6.4 × 10-3
  • 3.2 × 10-4
  • 3.2 × 10-2

Chemistry-Chemical Kinetics-1810.png

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    Chemistry-Chemical Kinetics-1812.png

  • Chemistry-Chemical Kinetics-1813.png

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The activation energy of a reaction is zero. The rate constant of the reaction ...
  • increase with increase of temperature
  • decrease with increase of temperature
  • decrease with decrease of temperature
  • is nearly independent of temperature
Which of the following is the fast reaction ?

  • Chemistry-Chemical Kinetics-1817.png
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    Chemistry-Chemical Kinetics-1818.png

  • Chemistry-Chemical Kinetics-1819.png

  • Chemistry-Chemical Kinetics-1820.png
Oxidation of oxalic acid by acidified KMnO4 is an example of autocatalysis. It is due to which of the following ?

  • Chemistry-Chemical Kinetics-1822.png
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    Chemistry-Chemical Kinetics-1823.png

  • Chemistry-Chemical Kinetics-1824.png

  • Chemistry-Chemical Kinetics-1825.png
Rate of chemical reaction can be kept constant...
  • by stirring the components
  • by keeping the temperature constant
  • both of the above
  • none of the above
For the reaction H2(g) + Br2(g) → 2HBr(g) the experimental data suggests, rate = K[H2][Br2]1⁄2.The molecularity and order of reaction respectively for the reaction is
  • 2, 2
  • 2)
    Chemistry-Chemical Kinetics-1831.png

  • Chemistry-Chemical Kinetics-1832.png

  • Chemistry-Chemical Kinetics-1833.png
The rate of reaction for Cl3 C CHO + NO → CHCl3 + NO + CO is given by equation, rate = K[Cl3 C CHO][NO]. If concentration is expressed in mole litre-1, the unit of K are
  • litre2 mole-2 sec-1
  • mole litre-1 sec-1
  • litre mole-1 sec-1
  • sec-1
According to the Arrhenius equation a straight line is to be obtained by plotting the logarithm of the rate constant of a reaction against ...
  • T
  • log T
  • 1/T
  • log 1/T

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    Chemistry-Chemical Kinetics-1837.png

  • Chemistry-Chemical Kinetics-1838.png

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Chemistry-Chemical Kinetics-1841.png
  • sec-1
  • sec-1 mole L-1
  • sec-1 mole-1 L
  • sec-1 mole-2 L2
The rate of the gaseous reaction is equal to K[A][B]. The volume of the vessel is suddenly reduced to one forth of the initial volume. The rate of reaction would be ...

  • Chemistry-Chemical Kinetics-1842.png
  • 2)
    Chemistry-Chemical Kinetics-1843.png

  • Chemistry-Chemical Kinetics-1844.png

  • Chemistry-Chemical Kinetics-1845.png
For reaction Y2 + 2Z → product, rate controlling step is Y + 1⁄2 Z → Q. If the concentration of Z is doubled, the rate of reaction will be
  • remain the same
  • become four times
  • become 1.414 times
  • become double
The rate law for a reaction given by Rate = K[A]n [B]m. On doubling the concentration of A and halving the concentration of B, the ratio of the new rate of the earlier rate of the reaction will be as
  • m + n
  • n - m
  • 2(n - m)

  • Chemistry-Chemical Kinetics-1847.png
For a first order reaction A → Products, the concentration of A changes from 0.1 M to 0.025 M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M is
  • 1.73 × 10-4 M min-1
  • 1.73 × 10-5 M min-1
  • 3.47 × 10-4 M min-1
  • 3.47 × 10-5 M min-1
In the reaction 2N2O5 → 4NO2 + O2 , initial pressure is 500 atm and rate constant K is 3.38 10-5 sec-1. After 10 minutes the final pressure of N2O5 is
  • 490 atm
  • 250 atm
  • 480 atm
  • 420 atm
The rate constants K1 and K2 for two different reactions are 1016.e-2000/T and 1015.e-1000/T respectively. The temperature at which K1 = K2 is
  • 1000 K
  • 2)
    Chemistry-Chemical Kinetics-1851.png
  • 2000 K

  • Chemistry-Chemical Kinetics-1852.png

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    Chemistry-Chemical Kinetics-1856.png

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  • 0.10 mol L-1 s-1
  • 2.6 × 10-2 mol L-1 s-1
  • 5.2 × 10-2 mol L-1 s-1
  • 6.5 × 10-3 mol L-1 s-1

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    Chemistry-Chemical Kinetics-1864.png

  • Chemistry-Chemical Kinetics-1865.png

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  • 1 × 10-4
  • 5 × 10-4
  • 1 × 10-3
  • 5 × 10-3

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    Chemistry-Chemical Kinetics-1872.png

  • Chemistry-Chemical Kinetics-1873.png

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For a reaction 1/2A → 2B, rate of disappearance of ‘A’ is related to the rate of appearance of B by the expression

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    Chemistry-Chemical Kinetics-1877.png

  • Chemistry-Chemical Kinetics-1878.png

  • Chemistry-Chemical Kinetics-1879.png

Chemistry-Chemical Kinetics-1881.png

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    Chemistry-Chemical Kinetics-1883.png

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  • Chemistry-Chemical Kinetics-1885.png

Chemistry-Chemical Kinetics-1887.png

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    Chemistry-Chemical Kinetics-1889.png

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  • 2.2 × 10-3
  • 1.1 × 10-3
  • 4.4 × 10-3
  • 5.5 × 10-3

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    Chemistry-Chemical Kinetics-1897.png

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Chemistry-Chemical Kinetics-1901.png
  • 0.0093 mol L-1 s-1
  • 0.012 mol L-1 s-1
  • 0.033 mol L-1 s-1
  • 0.040 mol L-1 s-1
For a first order reaction of k = 6.2 × 10-5 s-1, t3/4 will be
  • 4.65 × 10-5 s
  • 2.24 × 10-4 s
  • 2.24 × 10-5 s
  • 8.27 × 10-5 s
0:0:1


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