JEE Questions for Chemistry Chemical Kinetics Quiz 2 - MCQExams.com

Which one of the following is wrong about molecularity of a reaction?
  • It may be whole number of fractional
  • It is calculated from reaction mechanism
  • It is the number of molecules of the reactants taking part in a single step chemical reaction
  • It is always equal to the order of elementary reaction
In the synthesis of ammonia by Haber process, if 60 moles of ammonia is obtained in one hour, then the rate of disappearance of nitrogen is
  • 30 mol/min
  • 6 mol/min
  • 0.5 mol/min
  • 60 mol/min
The conversion of A to B follows second order kinetics, doubling the concentration of A will increase the rate of formation of B by a factor of
  • 4
  • 2
  • 1/4
  • 1/2
75% of a first order reaction is completed in 30 min. What is the time required for 93.75% completion of the reaction (in minutes) ?
  • 45
  • 120
  • 90
  • 60
Decay of 92U235 is ..... order reaction
  • zero
  • first
  • second
  • third
The half-life of two samples are 0.1 and 0.4 seconds. Their respective concentration are 200 and 50 respectively. What is the order of reaction?
  • 0
  • 2
  • 1
  • 4
The time required for 100% completion of a zero order reaction is
  • ak
  • 2)
    Chemistry-Chemical Kinetics-1517.png

  • Chemistry-Chemical Kinetics-1518.png

  • Chemistry-Chemical Kinetics-1519.png
The rate of the reaction A → products, at the initial concentration of 3.24 × 10-2 M is nine times its rate at another initial concentration of 1.2 × 10-3 M. The order of the reaction is

  • Chemistry-Chemical Kinetics-1521.png
  • 2)
    Chemistry-Chemical Kinetics-1522.png

  • Chemistry-Chemical Kinetics-1523.png

  • Chemistry-Chemical Kinetics-1524.png

  • Chemistry-Chemical Kinetics-1525.png
For a first order reaction, the concentration changes from 0.8 to 0.4 in 15 min. The time taken for the concentration to change from 0.1 M to 0.025 M is
  • 30 min
  • 15 min
  • 7.5 min
  • 60 min

Chemistry-Chemical Kinetics-1528.png
  • eight times
  • double
  • quadruple
  • triple
For the reaction, 2A + B → C + D, the order of reaction is
  • one with respect to [B]
  • two with respect to [A]
  • three
  • Cannot be predicted
If a plot of log10 C versus t gives a straight line for a given reaction, then the reaction is
  • zero order
  • first order
  • second order
  • third order
After how many seconds will the concentration of the reactant in a first order reaction be halved if the rate constant is 1.155 × 10-3 s-1 ?
  • 600
  • 100
  • 60
  • 10
The half-life period of a first order reaction is 69.3 s. What is the rate constant ?
  • 0.01 s-1
  • 0.1 s-1
  • 1 s-1
  • 10 s-1
Consider a reaction; aG + bH → products
When concentration of both the reactants G and H is doubled, the rate increases by eight times. However, when concentration of G is doubled keeping the concentration of H fixed, the rate is doubled. The overall order of the reaction is,
  • 0
  • 1
  • 2
  • 3
Consider the reaction, 2A + B → products When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is
  • L mol-1 s-1
  • no unit
  • mol L-1 s-1
  • s-1
The rate of first order reaction is 1.5 × 10-2 mol L-1 min-1 at 0.5 M concentration of the reactant. The half-life of the reaction is
  • 0.383 min
  • 23.1 min
  • 8.73 min
  • 7.53 min
At 500 K, the half-life period of a gaseous reaction at an initial pressure of 80 kPa is 350 s. When the pressure is 40 kPa, the half-life period is 175 s. The order of the reaction is
  • zero
  • one
  • two
  • three
  • half
The rate law for a reaction between the substances A and B is 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 to the earlier rate of the reaction will be as

  • Chemistry-Chemical Kinetics-1537.png
  • (m + n)
  • (n - m)
  • 2(n - m)
The t1/2 of the first order reaction is
  • dependent of initial concentration
  • directly proportional to initial concentration
  • indirectly proportional to initial concentration
  • independent of initial concentration
Which one of the following statements is incorrect about the molecularity of a reaction?
  • Molecularity of a reaction is the number of molecules of the reactants present in the balanced equation
  • Molecularity of a reaction is the number of molecules in the slowest step
  • Molecularity is always a whole number
  • There is no difference between order and molecularity of a reaction
The reaction, 2N2O5 ⇌ 2N2O4 + O2 is
  • bimolecular and second order
  • unimolecular and first order
  • bimolecular and first order
  • bimolecular and zero order
Rate of a reaction can be expressed by the following rate expression, Rate = k[A ]2[B] , if concentration of A is increased by 3 times and concentration of B is increased by 2 times, how many times rate of reaction increases?
  • 9 times
  • 27 times
  • 18 times
  • 8 times
For the first order reaction half-life is 14 s, the time required for the initial concentration to reduce to 1/8 of its value is
  • (14)3 s
  • 28 s
  • 42 s
  • (14)2 s
Which one is not correct ?
  • Rate of zero order reaction depends upon initial concentration of reactant
  • Rate of zero order reaction does not depend upon initial concentration of reactant
  • t1/2 of first order reaction is independent of initial concentration of reactant
  • t1/2 of zero order reaction is dependent of initial concentration of reactant
A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will
  • remain unchanged
  • triple
  • increases by a factor of four
  • double
The rate constant for a first order reaction whose half-life, is 480 s is
  • 2.88 × 10-3 s-1
  • 2.72 × 10-3 s-1
  • 1.44 × 10-3 s-1
  • 1.44 s-1
For a reaction A + B → C + D, if the concentration of A is doubled without altering the concentration of B, the rate gets doubled. If the concentration of B is increased by nine times without altering the concentration of A, the rate gets tripled. The order of the reaction is
  • 2
  • 1
  • 3/2
  • 4/3
Find the two-third life (t2/3 ) of a first order reaction in which k = 5.48 × 10-14 per second
  • 201 × 1013 s
  • 2.01 × 1013 s
  • 201 × 1020 s
  • 0.201 × 1010 s
  • None of these
The unit of rate constant of second order reaction
  • t-1
  • conc-1 t-1
  • conc t-1
  • conc-2 t-1
0:0:1


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