Chemical Kinetics Question 326

Question: The reaction of $ A_2 $ and $ B_2 $ follows the equation $ A_2(g)+B_2(g)\to 2AB(g) $ The following data were observed
$ {{[A_2]}_0} $ $ {{[B_2]}_0} $ Initial rate of appearance of $ AB(g),(in,M{s^{-1}}) $
0.10 0.10 $ 2.5\times {10^{-4}} $
0.20 0.10 $ 5\times {10^{-4}} $
0.20 0.20 $ 10\times {10^{-4}} $

The value of rate constant for the above reaction is:

Options:

A) $ 2.5\times {10^{-4}} $

B) $ 2.5\times {10^{-2}} $

C) $ 1.25\times {10^{-2}} $

D) None of these

Show Answer

Answer:

Correct Answer: C

Solution:

[c] Order w.r.t. A = 1; order w.r.t. B = 1 $ Rate=\frac{1}{2}\frac{d(AB)}{dt}=K_{r}[A][B]; $

$ \frac{1}{2}\times ( 2.5\times 10^{4} )=k_{r}( 0.1)(0.1 ) $

$ k_{r}=1.25\times {10^{-2}} $



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