JEE Questions for Chemistry Chemical Kinetics Quiz 6 - MCQExams.com


Chemistry-Chemical Kinetics-1611.png
  • -0.2 × 10-4
  • 0.2 × 10-4
  • 0.1 × 10-4
  • 0.3 × 10-4
The reaction, 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) is carried out in a 1dm3 vessel and 2 dm3 vessel separately. The ratio of the reaction velocities will be
  • 1 : 8
  • 1 : 4
  • 4 : 1
  • 8 : 1

Chemistry-Chemical Kinetics-1614.png
  • 1.3 × 10-5 Ms-1
  • 0.5 × 10-4 Ms-1
  • 7.6 × 10-4 Ms-1
  • 2 × 10-3 Ms-1
  • 2.5 × 10-5 Ms-1
The half - life of two samples are 0.1 and 0.8 s. Their respective concentration are 400 and 50 respectively. The order of the reaction is
  • 0
  • 2
  • 1
  • 4

Chemistry-Chemical Kinetics-1617.png
  • 1.15 atm
  • 1.32 atm
  • 1.22 atm
  • 1.12 atm
In a first order reaction, the concentration of the reactant decrease from 0.6 M to 0.3 M in 15 min. The time taken for the concentration to change from 0.1 M to 0.025 M in minutes is
  • 1.2
  • 12
  • 30
  • 3
For a first order reaction, (A) → products, the concentration of A changes from 0.1 M to 0.025 M in 40 min. The rate of reaction when the concentration of A is 0.01 M is
  • 1.73 × 10-5 M/min
  • 3.47 × 10-4 M/min
  • 3.47 × 10-5 M/min
  • 1.73 × 10-4 M/min
2N2O5 ⇌ 4NO2 + O2.
If rate and rate constant for above reaction are 2.40 × 10-5 mol L-1 s-1 and 3 × 10-5 s-1 respectively, then calculate the concentration of N2O5.
  • 1.4
  • 1.2
  • 0.04
  • 0.8
Consider the following statements in respect of zero order reaction.
I. The rate of the reaction is independent of reactant concentration.
II. The rate of the reaction is independent of temperature.
III. The rate constant of the reaction is independent of temperature.
IV. The rate constant of the reaction is independent of reactant concentration.
Choose the correct statement/s.
  • Only I
  • I and II
  • III and IV
  • I and III
  • I and IV
For a first order reaction, the initial concentration of a reactant is 0.05 M. After 45 min it is decreased by 0.015 M. Calculate half reaction time (t1/2)
  • 88.84 min
  • 25.90 min
  • 78.72 min
  • 77.20 min
The concentration of R in the reaction R → P was measured as a function of time and the following data is obtained
Chemistry-Chemical Kinetics-1623.png
  • zero
  • first
  • second
  • third
The time for half-life period of a certain reaction A → products is 1 h. When the initial concentration of the reactant 'A', is 2.0 mol L-1 , how much time does it take for its concentration to come from 0.50 to 0.25 mol L-1 , if it is a zero order reaction ?
  • 4 h
  • 0.5 h
  • 0.25 h
  • 1 h

Chemistry-Chemical Kinetics-1626.png
  • zero
  • second
  • third
  • pseudo first order
For a reaction between gaseous compounds,
2A + B → C + D
the reaction rate = k [A] [B]. If the volume of the container is made 1/4 of the initial, then what will be the rate of reaction as compared to the initial rate ?
  • 16 times
  • 4 times
  • 1/8 times
  • 1/16 times
In the first order reaction, 75% of the reactant gets disappeared in 1.386 h. The rate constant of the reaction is
  • 3.0 ×10-3 s-1
  • 2.8 ×10-4 s-1
  • 17.2 ×10-3 s-1
  • 1.8 ×10-3 s-1

Chemistry-Chemical Kinetics-1630.png
  • 1
  • -1/2
  • -3/2
  • 2
A first order reaction has a rate constant 1.15 × 10-3 s-1. How long will 5g of this reactant take to reduce to 3 g ?
  • 444 s
  • 402 s
  • 442 s
  • None of these
The half-life period of a first order chemical reaction is 6.93 min. The time required for the completion of 99% of the chemical reaction will be (log 2 = 0.301)
  • 230.3 min
  • 23.03 min
  • 46.06 min
  • 460.6 min
What is the formula to find the value of t1/2 for a zero order reaction ?

  • Chemistry-Chemical Kinetics-1634.png
  • 2)
    Chemistry-Chemical Kinetics-1635.png

  • Chemistry-Chemical Kinetics-1636.png

  • Chemistry-Chemical Kinetics-1637.png
For fourth order reaction, what is the unit of k ?
  • (mol / L)-3 s-1
  • (mol / L)+3 s-1
  • (mol / L)-3 s
  • (mol / L)-3
The half-life period of a first order reaction is 1 min 40 s. Calculate its rate constant.
  • 6.93 × 10-3 min-1
  • 6.93 × 10-3 s-1
  • 6.93 × 10-3 s
  • 6.93 × 103 s

Chemistry-Chemical Kinetics-1641.png
  • 2
  • 1
  • 1 1⁄2
  • 0

Chemistry-Chemical Kinetics-1643.png
  • 3
  • 2
  • 1
  • 0
For a first order reaction, the half-life period is
  • dependent on the square of the initial concentration
  • dependent on first power of initial concentration
  • dependent on the square root of initial concentration
  • independent on initial concentration
For a zero order reaction, the plot of concentration of reactant versus time is (intercept refers to concentration axis)
  • linear with positive slope and zero intercept
  • linear with negative slope and zero intercept
  • linear with negative slope and non-zero intercept
  • linear with positive slope and non-zero intercept
  • a curve asymptotic to concentration axis

Chemistry-Chemical Kinetics-1647.png
  • k [2A] [B]
  • k [A]3 [B]
  • k [A] [B]3
  • k [A]2 [B]
A reaction involving A, B and C as reactants is found to obey the rate law, rate = k [A]x [B]y [C]z . When the concentrations of A, B and C are doubled separately, the rate is also found to increase two, zero and four times respectively. The overall order of the reaction is
  • 1
  • 2
  • 3
  • 4
For the reaction system,
2NO(g ) +O2(g)→ 2NO 2(g)
volume is suddenly reduced to half its value by increasing the pressure on it. If the reaction is of first order with respect to O2 and second order with respect to NO; the rate of reaction will
  • diminish to one-fourth of its initial value
  • diminish to one-eighth of its initial value
  • increase to eight times of its initial value
  • increase to four times of its initial value
The rate equation for the reaction 2A + B → C is found to be rate = k [A] [B] The correct statement in relation to this reaction is that the
  • unit of k must be s -1
  • t1/2 is a constant
  • rate of formation of C is twice the rate of disappearance of A
  • value of k is independent of the initial concentrations of A and B

Chemistry-Chemical Kinetics-1652.png
  • mol-1 L s-1
  • s-1
  • s
  • s-1 mol L -1
0:0:1


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