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Chemical Kinetics question

2007 · Q90
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Chemical Kinetics question

2007 · Q90

NEETChemistryChemical KineticsMCQ+4 / −1
The reaction of hydrogen and iodine monochloride is given as :
H2(g) + 2ICl(g) →\to→ 2HCl(g) + I2(g)
This reaction is of first order with respect to H2(g) and ICl(g),
following mechanisms were proposed.

Mechanism A :
     H2(g) + 2ICl(g) →\to→ 2HCl(g) + I2(g)
Mechanism B :
     H2(g) + ICl(g) →\to→ HCl(g) + HI(g) ; slow
     HI(g) + ICl(g) →\to→ HCl(g) + I2(g) ; fast

Which of the above mechanism(s) can be consistent with the given information about the reaction?
  1. A
    A and B both
  2. B
    Neither A nor B
  3. C
    A only
  4. D
    B only
View written solutionFree

Correct answer: D

The slow step is the rate determining step and it involves 1 molecule of H2(g) and 1 molecule of ICl(g) . Hence the rate will be,

r = k[H2(g)] [ICl(g)]

∴\therefore∴ The reaction is 1st order with respect to H2(g) and ICl(g).

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