JEE Main 2016 Chemistry question
Decomposition of follows a first order reaction. In fifty minutes the concentration of decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of reaches 0.05 M, the rate of formation of will be:
Answer: (4)
Solution
The concentration falls from 0.5 to 0.125 M, a factor of 4, which is two half-lives. Hence min and min, giving
k = = = 2.772×\ min^{-1}.
When M, the rate of its disappearance is
-{d[H_2\text{
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