Chemical Kinetics and Nuclear ChemistryHard
Question
A certain reaction A → B follows the given concentration (Molarity)-time graph. Which of the following statements is/are true ?
Options
A.The reaction is second order with respect to A.
B.The rate for this reaction at 20 s will be 7 × 10-3 M s-1.
C.The rate for this reaction at 80 s will be 1.75 × 10-3 M s-1.
D.The [B] will be 0.35 M at t = 60 s.
Solution
Use initial rate law method, let the reaction be first order,
So, k =
B. At t = 20 s, k1 =
= k1
⇒ Assumption is correct (k1 = k2)
Rate at 20 s = k[A] =
× 0.2
= 0.0063 ≈ 7 × 10-3 M s-1
Clearly, half life t1/2 = 20 s
D. In 60 s, number of life =
= 3
⇒ [B] at 60 s
= 0.4 - 0.4
= 0.35 M
So, k =
B. At t = 20 s, k1 =
= k1⇒ Assumption is correct (k1 = k2)
Rate at 20 s = k[A] =
× 0.2= 0.0063 ≈ 7 × 10-3 M s-1
Clearly, half life t1/2 = 20 s
D. In 60 s, number of life =
= 3⇒ [B] at 60 s
= 0.4 - 0.4
= 0.35 MCreate a free account to view solution
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