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Chemical Kinetics MHT-CET PYQ's

 

MHT-CET 2008  

1 . After how many seconds will the concentration of the reactant in a first order reaction be halved if the rate constant is 1.155 x 10^-3 s^-1

  • (A) 600 
  • (B) 100 
  • (C) 60 
  • (D) 10

MHT-CET 2009

 2. Which is a correct integrated rate equation?

  • (A) k = -2.303/t log a/(a - x)
  • (B) k = -2.303/t log (a - x)/a
  • (C) -d (a - x) = k dt
  • (D) All are integrated rate equations

3. For which order reaction, the unit of rate constant is time^-1 ?

  • (A) Zero order 
  • (B) First order 
  • (C) Second order 
  • (D)Third order 

MHT-CET 2010

4. The units of rate constant for first order reaction are 

  • (A) mol L-1 s-1
  • (B) s-1
  • (C) L mol-1 s-1
  • (D) L² mol-2 s-1
5. The first order integrated rate equation is 
  • (A) k = x/t
  • (B) k = -2.303/t log a/(a-x)
  • (C) k = 1/t ln a/(a-x)
  • (D) k = 1/t x/a(a-x)
MHT-CET 2011
 
6. In a multistep reaction, the overall rate of reaction is equal to the
  • (A) rate of slowest step 
  • (B) rate of fastest step
  • (C) average rate of various steps 
  • (D) the rate of last step
7. What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20°C to 35°C ? (R = 8.314 J mo1-1 K-1 
  • (A) 342 kJ mo1-1 
  • (B) 269 kJ mol-1 
  • (C) 34.7 kJ mol-1 
  • (D) 15.1 kJ mol-1 
MHT-CET 2014 
8. Rate law for the reaction A + B → product is rate = k [A]2 [B]. What is the rate constant if the rate of reaction at a given temperature is 0.22 Ms-1. when [A] = 1M and [B] = 0.25 M? 
  • (A) 3.52 M-2s-1 
  • (B) 0.88 M-2s-1 
  • (C) 1.136 M-2s-1 
  • (D) 0.05 M-2s-1 
MHT-CET 2015
 
9. For the reaction O3(g) + O(g) → 2O2(g) if the rate law expression is, rate = k [O3] [O] the molecularity and order of the reaction are respectively 
  • (A) 2 and 2 
  • (B) 2 and 1.33 
  • (C) 2 and 1 
  • (D) 1 and 2
10. The relationship between rate constant and half-life period of zero order reaction is given by 
  • (A) t1/2 = [A]02kt
  • (B) t1/2 = 0.693/k
  • (C) t1/2 = [A]/2k
  • (D) t1/2 = 2[A]0/k
11. Half-life period of a first order reaction. A → product is 6.93 hour. What is the value of rate constant? 
  • (A) 1.596 h-1
  • (B) 0.1 h-1
  • (C) 4.802 h-1
  • (D) 10 h-1
MHT-CET 2016 
 
12. The reaction takes place in two steps as 
i) NO2C(g) → NO2(g) + Cl(g)  ii) NO2Cl(g) + Cl(g) → NO2(g) + C12(g) Identify the reaction intermediate. 
  • (A)NO2Cl(g)
  • (B) NO2(g)
  • (C) Cl2(g) 
  • (D) Cl(g)
13. The rate constant and half-life of a first order reaction are related to each other as 
  • (A) t1/2 = 0.693/k
  • (B) t1/2 = 0.693 k
  • (C) k  = 0.693 t1/2 
  • (D) kt1/2 = 1/0.693
14. Average rate of reaction 2 SO2(g) + O2(g) → 2SO3(g) is written as
  • (A) △[SO2]/△t
  • (B) -△[O2]/△t
  • (C) 1/2△[SO2]/△t
  • (D) △[SO3]/△t
MHT-CET 2017
 
15. Which among the following reactions is an example of pseudo first order reaction?
  • (A) Inversion of cane sugar 
  • (B) Decomposition of H2O2
  • (C) Conversion of cyclopropane to propene 
  • (D) Decomposition of N2O5
16. Which among the following equations represents Arrhenius equation?
  • (A) k = A.eEa/RT
  • (B) k = A.eRT/Ea
  • (C) k = A/eEa/RT
  • (D) k = A/eRT/Ea
17. The rate constant for a first order reaction 7.0 x 10^-4 s^-1. If initial concentration of reactant is 0.080, what is the half-life of reaction?
  • (A) 990 s
  • (B) 79.2 s
  • (C) 12375 s
  • (D) 10.10 x 10^-4
MHT-CET 2018
 18. A certain reaction occurs in two steps as
i) 2SO2(g) + 2NO2(g) → 2SO3(g) + 2NO(g)  ii) 2NO(g) + O2(g) → 2NO2(g)
in the reaction,
  • (A) NO2(g) is intermediate 
  • (B) NO(g) is intermediate 
  • (C) NO(g) is catalyst 
  • (D) O2(g) is intermediate 
19. Slope of the straight line obtained by plotting log10k against 1/T represents what term?
  • (A) -Ea 
  • (B) -2.303 Ea/R
  • (C) -Ea/2.303 R 
  • (D) -Ea/R 
MHT-CET 2019 
 
20. For the elementary reaction 2SO2(g) + O2(g)  → 2SO3(g), identify the correct among the following relations:
  • (A) +d[SO3(g)]/dt = -2d[O2(g)]/dt
  • (B) +d[SO2(g)]/dt = -d[O2(g)]/dt
  • (C) +1/2d[SO3(g)]/dt = d[SO2(g)]/dt
  • (D) -d[SO2(g)]/dt = -d[O2(g)]/dt
21. Which among the following reaction is an example of a zero order reaction? 
  • (A) 2NH3 → N2(g) + 3H2 
  • (B) C12H22O11(aq.) + H2O(l) → C6H12O6(aq.) + C6H12O6(aq.)
  • (C) H2(g) + I2(g) → 2HI(g)
  • (D) 2H2O2(l) → 2H2(l) + O 2(g)
22. The activation energy of a reaction is zero. Its rate constant at 280 K is 1.6 x 10^-6 s^-1, the rate constant at 300 K is 
  • (A) 1.6 x 10^-6 s^-1
  • (B) 1.6 x 10^-5 s^-1
  • (C) 3.2 x 10^-6 s^-1
  • (D) Zero
23. For a chemical reaction rate law is. rate = k [A]² [B]. If [A] is doubled at constant [B], the rate of reaction 
  • (A) increases by a factor of 4 
  • (B) increases by a factor of 3 
  • (C) increases by a factor of 8 
  • (D) increases by a factor of 2 
24. For the elementary reaction, 3 H2(g) + N2(g) → 2NH3(g), identify the correct relation among the following relations.
  • (A) -3/2d[H2(g)]/dt = d[NH3(g)]/dt
  • (B) d[NH3(g)]/dt = -1/3 d[H2(g)]/dt
  • (C) -2/3d[H2(g)]/dt = d[NH3(g)]/dt
  • (D) -[H2(g)]/dt = d[NH3(g)]/dt
25. The integrated rate equation for first order reaction, A  → Product, is 
  • (A) k = 2.303 t log10[A]0/[A]t
  • (B) k = –1/t ln[A]t/[A]0
  • (C) k = 2.303/t + log10[A]0/[A]t
  • (D) k = 1/t ln[A]t/[A]0
  •  
    26. Order of which among the following reactions is NOT one? 
    • (A) 2H2O2(l) → 2H2O(l) + O2(g)
    • (B) Cyclopropane  → CH3 -- CH == CH2(g)
    • (C) 2N2O5(g)  → 2NO2(g) + O2(g)
    • (D) CHCl3(g) + Cl2(g) → CCl4(g) + HCl(g)
    27. Consider the reaction 2A + B → product. When conc. of 'B' alone was doubled, the half-life, is not change. When conc. of 'A' alone was doubled, the rate increases by two times, order of of reaction is
    • (A) 2 
    • (B) 1.5 
    • (C) 1 
    • (D) 0
    28. Consider the reaction 2A + 2B  → C + 2D, if concentration of A is doubled at constant [B], rate increases by a factor 4. If concentration B is doubled at constant [A] the rate is doubled. Rate law of the reaction is 
    • (A) rate =  k[A]2 [B]
    • (B) rate = k[A] [B]2
    • (C) rate = k[A]2 [B]2 
    • (D) rate = k[A] [B]
    29. If the half-life period of a first order reaction is 200 minutes, the rate constant will be 
    • (A) 9.605 x 10^-2 min^-1 
    • (B) 3.465 x 10^-3 min^-1 
    • (C) 1.374 x 10^-3 min^-1
    • (D) 288.6 min^-1
    30. If the rate of reaction is expressed as,  -1/3d[A]/dt = -1/2d[B]/dt = d[C]/dt, the reaction is
    • (A) 3A + 2B → C 
    • (B) 2B  → 3A + C 
    • (C) 2B + C  → 3A 
    • (D) 3A → 2B + C 
    31. A  → B is first order reaction with rate equal to 6.6 x 10^-5 M s^-1. When [A] is 0.6 M, rate constant of the reaction is 
    • (A) 9 x 10^-5 s^-1
    • (B) 9 x 10^-4 s^-1
    • (C) 1.1 x 10^-4 s^-1
    • (D) 1.1 x 10^-5 s^-1
    MHT-CET 2020 
     
    32. Which of the following is a character of catalyst? 
    • (A) It increases the rates of both forward and backward reactions equally in reversible reaction
    • (B) It increases the activation energy of reactants 
    • (C) It affects the energies of reactants and products of the reaction 
    • (D) It changes the position of equilibrium 
    33. In the reaction. N2 is + 3H2 → 2NH3, the rate of disappearance of H2 is 0.02 M/s. The rate of appearance of NH3 is
    • (A) 0.0133 M/s 
    • (B) 0.004 M/s 
    • (C) 0.032 M/s
    • (D) 0.023
    34. Which among the following is correct when energy of activation, Ea of the catalyzed reaction decreases at constant temperature and for same concentration? 
    • (A) e-Ea/RTdecreases 
    • (B) -Ea/RT decreases 
    • (C) K decreases
    • (D) Ea/RT decreaces
     35. Half-life of first order reaction is 20 minutes. What is the time taken to reduce the initial concentration of the reactant to 1/10 th ? 
    • (A) 66.56 min 
    • (B) 6.6 min 
    • (C) 150 min 
    • (D) 79.68 min
    36. The rate law for the reaction 2NO(g) + O2(g) → 2NO2(g) is rate = k[NO]²[O2], then which
    among the following is correct?
    • (A) The reaction is first order in O2, first order in NO and second order overall
    • (B) The reaction is second order in NO, zero order in O2 and second order overall 
    • (C) The reaction is second order in NO, first order in O2 and third order overall
    • (D) The reaction is zero order overall
    37. In a first order reaction 87.5% of reactant is converted into product in 15 minutes. The rate constant for the reaction is given by
    • (A) 5/0.693 min^-1
    • (B) 0.693/15 min^-1
    • (C) 0.693 x 5 min^-1
    • (D) 0.693/5 min^-1
    38. The half-life of a first order reaction is 6.0 hour. How long will it take for the concentration of reactant to decrease from 0.4 M to 0.12 M?
    • (A) 10.42 h
    • (B) 9.51 h 
    • (C) 30.36 h 
    • (D) 4.25 h 
    39. For the first order reaction A → B, the rate constant is 0.25 s^-1, if the concentration of A is reduced to half, the value of rate constant will be 
    • (A) 0.25 s^-1
    • (B) 0.30 s^-1
    • (C) 2.25 s^-1
    • (D) 0.075 s^-1
    40. For the reaction 4NH3 + 5O2 → 4NO + 6H2O, the rate of disappearance of NH3 is 3.6 x 10^-3M/s. What is the rate of formation of water? 
    • (A) 6.0 x 10^-4 M/s
    • (B) 5.4 x 10^-3 M/s 
    • (C) 3.6 x 10^-3 M/s 
    • (D) 4.0 x 10^4 M/s 
    41. The rate law for the reaction A + B + C → Product is expressed as Rate = k[A]² [B]1 [C]0. What is the overall order of the reaction? 
    • (A) 3 
    • (B) 1 
    • (C) 2
    • (D) 0
    42. The reaction N205 → 2NO2 + 1/2O2 is first order in N205 having rate constant 6.2 x 10^-4 s^-1. What is the value of rate of reaction when concentration of N2O5 is 1.25 mol L^-1?
    • (A) 7.75 x 10^-4 mol L^-1 s^-1
    • (B) 8.15 x 10^-4 mol L^-1 s^-1
    • (C) 4.96 x 10^-4 mol L^-1 s^-1
    • (D) 2.01 x 10^-4 mol L^-1 s^-1
    43. The rate constant for first order reaction is 0.02232 min^-1. Calculate the time required for 75% completion of the reaction. 
    • (A) 62.12 min 
    • (B) 38.31 min 
    • (C) 48.12 min 
    • (D) 12.77 min 
    44. Which among the following is an example of zero order reaction? 
    • (A) Hydrolysis of CH3COOCH3 
    • (B) inversion of C12H22O11
    • (C) Decomposition of N2O in presence of catalyst 
    • (D) Decomposition of N2O5 
    45. What is the unit of rate constant for the zero order reaction? 
    • (A) t^-1 
    • (B) mol dm³ t^-1
    • (C) mol dm^-3 t^-1
    • (D) mol dm^-3 t
    46. For first order reaction the slope of the graph of log[A]t Vs. time is equal to
    • (A) k
    • (B) -k
    • (C) -k/2.303
    • (D) k/2.303
    47. What is the order of reaction for decomposition of gaseous acetaldehyde?
    • (A) 0
    • (B) 2
    • (C) 1.5
    • (D) 1
    48. If concentration of reactant 'A' is increased by 10 times, the rate of reaction becomes 100 times. What is the order of reaction if rate law is, rate = k[A]x
    • (A) 2
    • (B) 1
    • (C) 3
    • (D) 4
    49. A first order reaction has rate constant 1 x 10^-2 s^-1. What time will it take for 20 g of reactant to reduce to 5 g?
    • (A) 138.6 s
    • (B) 238.6 s 
    • (C) 693.0 s 
    • (D) 346.5 s
    50. What is the value of rate constant of first order reaction, if it takes 15 minutes for consumption of 20% of reactants? 
    • (A) 1.07 x 10^-2 min^-1
    • (B) 1.48 x 10^-2 min^-1 
    • (C) 1.84 x 10^-2 min^-1 
    • (D) 1.38 x 10^-2 min^-1
    51. A first order reaction has a rate constant 0.00813 min^-1, how long will it take for 60% completion? 
    • (A)112.7 min 
    • (B) 56.35 min 
    • (C) 62.77 min 
    • (D) 98.7 min
    52. Half-life of first order reaction X → Y + Z is 3 minutes. What is the time required to reduce the concentration of 'X' by 90 % of it's initial concentration? 
    • (A) 9.969 minutes 
    • (B) 4.12 minutes 
    • (C) 9.105 minutes 
    • (D) 12.05 minutes 
    53. A first order reaction is 25% completed in 40 minutes. What is the rate constant k for reaction? 
    • (A) 2.303/40 x log1/4 
    • (B) (2.303 x log 1.33)/40
    • (C) (2.303 x log 4)/120
    • (D) 2.303 x log 4/3
    54. For first order reaction the concentration of reactant decreases form 0.2 to 0.1 M in 100 minutes What is the rate constant of the reaction? 
    • (A) 144.3 min^-1 
    • (B) 6.93 min^-1 
    • (C) 69.3 min^-1
    • (D) 6.93 x 10^-3 min^-1
    55. A first order reaction is 75% completed in 60 minutes, the time required for it's 50% completion is 
    • (A) 30 min 
    • (B) 60 min 
    • (C) 120 min 
    • (D) 40 min 
    56. What is the molecularity and order of the following reaction if rate law is, rate = k[O3][O] respectively?
    O3(g) + O(g) → 2O2(g)
    • (A) 3 and 1 
    • (B) 3 and 2 
    • (C) 4 and 2
    • (D) 2 and 2
    57. For a first order reaction, A → B, if [A] = 1 M and rate is 4 x 10^-2 M s^-1. What is the rate constant of the reaction? 
    • (A) 4 x 10^-2 s^-1 
    • (B) 0.4 x 10^-2 s^-1 
    • (C) 2 x 10^-2 s^-1
    • (D) 2.5 x 10^-5 s^-1
    58. For the reaction, 2NOBr(g) → 2NO(g) + Br2(g), rate law is r = k [NOBr]².
    If rate constant is 1.62 Ms^-1 and concentration of NOBr is 2.00 x 10^-3M, what is the rate of reaction?
    • (A) 2.46 x 10^-6 Ms^-1
    • (B) 5.24 x 10^-6 Ms^-1
    • (C) 6.48 x 10^-6 Ms^-1
    • (D) 4.05 x 10^-5 Ms^-1
    59. In the reaction 2SO2 + O2 → 2SO3 the rate of appearance of SO3 is 4 x 10^-4 M/s, the rate of disappearance of O2 is 
    • (A) 1.0 x 10^-4 M/s 
    • (B) 4.0 x 10-4 M/s 
    • (C) 2.0 x 10^-4
    • (D) 6.0 x 10^-4 M/s
    60. Which among the following is an example of pseudo first order reaction? 
    • (A) 2N2O5(g) → 4NO2(g) + O2(g)
    • (B) CH2 --CH2-- CH2 → CH3 -- CH= CH2
    • (C) H2O2(l) → 2H2)(l) + O2(g)
    • (D) CH3COOCH3(aq.) + H2O → CH3COOH(aq.) + CH3OH(aq.)
    61. Which is the average rate of reaction when the change in concentration of product is 0.05 M in 20 seconds?
    • (A) 4.0 m/s
    • (B) 0.05 M/s 
    • (C) 0.0025 M/s 
    • (D) 1.0 M/s 
    62. In the reaction A + B2 → AB + B, the rate of reaction is direct, proportional to the cocentration of A and independent on the concentration of B2. What is the rate law expression? 
    • (A) rate = k[A]
    • (B) rate = k[B2]
    • (C) rate = k[A][B2]
    • (D) rate = K[A]2[B2]
    63. The rate for the reaction is r1 = k[A][B]. If the concentration of A is doubled and that of B is halved, the new rate is r2 then what is the ratio of r2/r1?
    • (A) 2^( a – b)
    • (B) a - b
    • (C) a + b 
    • (D) 1/2^(a+b)
    64. The reaction 2NO2Cl(g) → 2NO2(g) + Cl2(g) takes place in two steps its 
    (i) NO2Cl(g) → 2NO2(g) + Cl2(g)
    (ii) NO2Cl(g) + Cl(g) → NO2(g) + Cl2(g)
    Identify the reaction intermediate. 
    • (A) NO2(g) 
    • (B) NO2Cl(g)
    • (C) Cl(g) 
    • (D) C12(g)
    65.1n the reaction 2SO2(g) + O2(g) → 2SO3(g), the rate of disappearance of SO2 is 1.28 x 10^-5 M/s. What is the rate of appearance of SO3? 
    • (A) 2.56 x 10^-5 M/s 
    • (B) 1.25 x 10^-5 M/s 
    • (C) 0.64 x 10^-5 M/s 
    • (D) 0.32 x 10^-5 M/s
     
    66. A first order reaction takes 40 minutes for 30% decomposition. What is the half-life of reaction? 
    • (A) 59.5 min 
    • (B) 77.8 min 
    • (C) 67.8 min 
    • (D) 82.2 min 
    67. A certain zero order reaction is 50% completed in 10 minutes. What percentage does the reaction completes after 15 minutes?
    • (A) 65%
    • (B) 25%
    • (C) 75% 
    • (D) 60%
    68. In a reaction N2(g) + 3H2(g) → 2NH3(g), if the rate of disappearance of N2(g) is 2.6 x 10^-4 M/s, the rate of disappearance of H2(g) in M/s is 
    • (A) 8.6 x 10^-4 M/s 
    • (B) 5.2 x 10^-4 M/s 
    • (C) 2.6 x 10^-4 M/s 
    • (D) 7.8 x 10-4 M/s 
    69. Which is the unit of rate constant for the first order reaction if time is expressed in seconds? 
    • (A) mol^-1 dm³ s^-1 
    • (B) s^-1 
    • (C) mol dm^-3 s^-1 
    • (D) mol dm^-3 s 
    70. Reaction given below follows first order kinetics: 2 N2O2 → 4NO2 + O2
    Calculate rate constant of reaction if concentration of N2O2 is 0.05 M and rate of reaction is 
    1.5 x 10^-6 mol L^-1 s^-1
    • (A) 2.5 x 10^-5 s^-1
    • (B) 3.0 x 10^-5 s^-1 
    • (C) 1.5 x 10^-5 s^-1
    • (D) 2.0 x 10^-5 s^-1
    71. A certain zero order reaction has rate constant 0.025 M s^-1. What will be the concentration of reactant 'A' after 15 seconds, if initial concentration is 0.50 M? 
    • (A) 0.50 M 
    • (B) 0.125 M
    • (C) 0.375 M
    • (D) 0.060 M
    72. The reaction A + B →  P, is second order in A and first order in B. What is the rate law for the reaction?
    • (A) Rate = k[A] [B]
    • (B) Rate = k[A]² [B]^1/2
    • (C) Rate = k[A]² [B] 
    • (D) Rate = k[A] [B]²
    73. A first order reaction is 50 % completed in 50 minutes. What is the rate constant of the reaction?
    • (A) 7.215 x 10^-1 min^-1
    • (B) 3.465 x 10^-2 min^-1
    • (C) 1.386 x 10^-2 min^-1
    • (D) 1.386 x 10^-1 min^-1
    74. A first order reaction takes 40 minutes for 30% completion. Calculate the half-life of reaction
    • (A) 77.7 min
    • (B) 23.1 min
    • (C) 42.7 min
    • (D) 57.8 min
    75. Rate constant for zero order reaction is 2 x 10^-2 mol^-1 s^-1. If the concentration of the reactant after 25 sec. is 0.5 M, what is the initial concentration of reactant?
    • (A) 0.125 M 
    • (B) 0.5 M 
    • (C) 1.25 M 
    • (D) 1.0 M 
    76. The slope of a graph. log [A]t versus 't' for a first order reaction is - 2.5 x 10^-3 s^-1. The rate constant for the reaction is 
    • (A) - 2.5 x 10^-3 s^-1
    • (B) 2.5 x 10^-3 s^-1
    • (C) 1.086 x 10^-3 s^-1
    • (D) 5.757 x 10^-3 s^-1
    77(78). A first order reaction, A → B takes 100 minutes for it's 90% completion. What is the rate constant of reaction? 
    • (A) 0.0460 min^-1 
    • (B) 0.0230 min^-1
    • (D) 0.2303 min^-1
    • (D) 0.4606 min^-1
    78. 0.0210 M solution of N2O5 is allowed to decompose at 43°C. How long will it take to reduce 0.0150M ? (Given k = 6.0 x 10^-4 sec^-1)
    • (A) 3364 sec 
    • (B) 360.0 sec 
    • (C) 560.0 sec
    • (D) 5600 sec
    79. The rate of first order reaction A → B is 6.3 x 10^-6 M s^-1, if [A] = 0.3 M, what is the rate constant of the reaction?
    • (A) 1.3 x 10^-5 s^-1
    • (B) 2.1 x 10^-5 s^-1 
    • (C) 1.2 x 10^-5 s^-1
    • (D) 1.6 x 10^-5 s^-1 
    80. For zero order reaction, when [A]t is plotted against time (t), the slope of the straight line obtained is equal to 
    • (A) -k 
    • (B) -kt 
    • (C) k
    • (D) [A]0
    81. A first order reaction is 50 % completed in 16 minutes. The percentage of reactant that will react in 32 minutes is 
    • (A) 75 % 
    • (B) 12-5%
    • (C) 25%
    • (D) 100%
    82. Consider the reaction; 2N2O5(g) → 4NO2(g) + O2(g). What is the rate of reaction, when the concentration of NO2 increases to 5.2 x 10^-3 M in 100 sec?
    • (A) 2 x 10^-5 M/s
    • (B) 7.6 x 10^-4 M/s
    • (C) 5 x 10^-4 M/s
    • (D) 1.3 x 10^-5 M/s
    83. For the reaction 2A + B → 3C + D, which among the following is NOT the correct rate law expression ?
    • (A) -d[A]/2dt
    • (B) -d[B]/dt
    • (C) d[D]/dt
    • (D) -d[C]/3dt
    84. The time required to decompose SO2Cl2 to half of it's initial amount is 60 minutes. Calculate rate constant for the first order reaction.
    • (A) 4.158 x 10^-2 min^-1
    • (B) 2.651 x 10^-2 min^-1
    • (C) 1.155 x 10^-2 min^-1
    • (D) 1.551 x 10^-2 min^-1
    85. The rate constant for the first order reaction is 1.15 x 10^-3 s^-1. How long will 5g of the reactant take to reduce to 3g?
    • (A) 414 sec
    • (B) 444 sec
    • (C) 424 sec
    • (D) 434 sec
    86. When the temperature of first order reaction increases then according to Arrhenius equation which among the following is correct?
    • (A) e - Ea/RT decreases
    • (B) Ea/RT increases
    • (C) -Ea/RT decreases
    • (D) k decreases

     

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