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Chemical Kinetics · Question 54

AIPMT 2009MCQEasy📈 Topic in 38% papers+4−1
1

For the reaction A + B products, it is observed that (i) on doubling the initial concentration of A only, the rate of reaction is also doubled and (ii) on doubling the initial concentration of both A and B, there is a change by a factor of 8 in the rate of the reaction. The rate of this reaction is given by

  1. rate = k[A]2[B]2
  2. rate = k[A][B]2
  3. rate = k[A][B]
  4. rate = k[A]2[B]

Answer

(2) rate = k[A][B]2

Solution

Let rate = k[A]x[B]y

doubling [A] alone doubles the rate 2x = 2 x = 1

doubling both makes the rate 8 times 2x 2y = 8

2 2y = 8 y = 2

rate = k[A][B]2

Answer: (2)

AIPMT 2009

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2

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

  1. 2000 K
  2. 10002.303 K
  3. 1000 K
  4. 20002.303 K
AIPMT 2008
3

The bromination of acetone that occurs in acid solution is represented by this equation. CH3COCH3(aq) + Br2(aq) CH3COCH2Br(aq) + H+(aq) + Br-(aq) These kinetic data were obtained for given reaction concentrations. array|c|c|c|c| [CH3COCH3], M & [Br2], M & [H+], M & Initial rate, disappearance of Br2, M s-1 \ 0.30 & 0.05 & 0.05 & 5.7 10-5 \ 0.30 & 0.10 & 0.05 & 5.7 10-5 \ 0.30 & 0.10 & 0.10 & 1.2 10-4 \ 0.40 & 0.05 & 0.20 & 3.1 10-4 \ array Based on these data, the rate equation is

  1. Rate = k[CH3COCH3][Br2][H+]2
  2. Rate = k[CH3COCH3][Br2][H+]
  3. Rate = k[CH3COCH3][H+]
  4. Rate = k[CH3COCH3][Br2]
AIPMT 2008
4

If 60% of a first order reaction was completed in 60 minutes, 50% of the same reaction would be completed in approximately (log 4 = 0.60, log 5 = 0.70)

  1. 45 minutes
  2. 60 minutes
  3. 40 minutes
  4. 50 minutes
AIPMT 2007
5

In a first-order reaction A B, if k is rate constant and initial concentration of the reactant A is 0.5 M, then the half-life is

  1. 2k
  2. 2k 0.5
  3. 2k
  4. 0.6930.5k
AIPMT 2007
6

The reaction of hydrogen and iodine monochloride is given as: H2(g) + 2ICl(g) 2HCl(g) + I2(g) This reaction is of first order with respect to H2(g) and ICl(g). The following mechanisms were proposed. Mechanism A: H2(g) + 2ICl(g) 2HCl(g) + I2(g) Mechanism B: H2(g) + ICl(g) HCl(g) + HI(g); slow HI(g) + ICl(g) HCl(g) + I2(g); fast Which of the above mechanism(s) can be consistent with the given information about the reaction?

  1. A and B both
  2. Neither A nor B
  3. A only
  4. B only
AIPMT 2007
7

Consider the reaction : N2(g) + 3H2(g) 2NH3(g) The equality relationship between d[NH3]dt and - d[H2]dt is

  1. d[NH3]dt = - d[H2]dt
  2. d[NH3]dt = - 13 d[H2]dt
  3. + d[NH3]dt = - 23 d[H2]dt
  4. + d[NH3]dt = - 32 d[H2]dt
AIPMT 2006
8

For the reaction, 2A + B 3C + D, which of the following does not express the reaction rate?

  1. - d[A]2dt
  2. - d[C]3dt
  3. - d[B]dt
  4. d[D]dt
AIPMT 2006
9

The rate of reaction between two reactants A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is

  1. 2
  2. -2
  3. 1
  4. -1
AIPMT 2005
10

For a first order reaction A B the reaction rate at reactant concentration of 0.01 M is found to be 2.0 10-5 mol L-1 s-1. The half-life period of the reaction is

  1. 30 s
  2. 220 s
  3. 300 s
  4. 347 s
AIPMT 2005
11

The rate of a 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

  1. 0.383 min
  2. 23.1 min
  3. 8.73 min
  4. 7.53 min
AIPMT 2004

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