Chemical Kinetics Question 172
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}} $
BETA
