Chemical Kinetics Question 322
Question: Consider the reaction: $ N_2(g)+3H_2(g)\to 2NH_3(g) $ The equality relationship between $ \frac{d[NH_3]}{dt} $ and $ -\frac{d[H_2]}{dt} $ is
Options:
A) $ +\frac{d[NH_3]}{dt}=-\frac{2}{3}\frac{d[H_2]}{dt} $
B) $ +\frac{d[NH_3]}{dt}=-\frac{3}{2}\frac{d[H_2]}{dt} $
C) $ \frac{d[NH_3]}{dt}=-\frac{d[H_2]}{dt} $
D) $ \frac{d[NH_3]}{dt}=-\frac{1}{3}\frac{d[H_2]}{dt} $
Show Answer
Answer:
Correct Answer: A
Solution:
[a] If we write rate of reaction in terms of concentration of $ NH_3 $ and $ H_2 $ then Rate of reaction $ =\frac{1}{2}\frac{d[NH_3]}{dt}=-\frac{1}{3}\frac{d[H_2]}{dt} $ So, $ =\frac{d[NH_3]}{dt}=-\frac{2}{3}\frac{d[H_2]}{dt} $
