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The rate of a first order reaction is 0.04 mol L-1 s-1 at 10 minutes and 0.03 mol L-1 s-1 at 20 minutes after initiation. Half life of the reaction is minutes. (Given 2 = 0.3010, 3 = 0.4771)
24
First order: rate = k[A] ⇒ rate [A]
k = 2.303(20-10) min 0.040.03 = 2.30310 43
t1/2 = 0.693k = 2.303 2k
= 10 2 4 - 3
= 10 0.30100.6020 - 0.4771 = 3.0100.1249
= 24.1 min ≈ 24
Answer: 24
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