A) 1
B) Zero
C) 2
D) 3
Correct Answer: A
Solution :
50% of a reaction occurs in 100 second and 75% of the reaction occurs in 200 second, the order of this reaction is 1. Let the initial reactant concentration is 1 M. In first 100 seconds, reactant concentration is reduced to 50% or \[1\times \frac{50}{100}=0.5\,M.\] In second 100 seconds (total 200 seconds from start), reactant concentration is reduced to\[100-75=25%\]or \[1\times \frac{25}{100}=0.25\,M.\] Thus we observe that after each 100 second period, the reactant concentration is reduced to one half. Hence, 100 second is half-life period and is independent of reactant concentration. This is characteristic of first order reaction.
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