1. The reaction A → B + C is zero order with respect to A. When [A]0 = 0.544 M, the reaction is 28 % complete at 91.5 min. Calculate the half-life for this reaction.
2. Consider the following reaction. Calculate the value of the rate constant..
2 A + B →→ 2 C
A B C Rate
Trial 1 0.64 0.56 0.012 7.463
Trial 2 1.28 0.56 0.012 14.926
Trial 3 0.64 1.12 0.012 14.926
Trial 4 0.1 0.4 0.012 ?
we have:
[A]o = 0.544 M
28 % is completed. So, remaining is 72 %
[A] = 72 % of 0.544 M
= 72*0.544/100
= 0.392 M
t = 91.5 min
use integrated rate law for 0 order reaction
[A] = [A]o - k*t
0.392 = 0.544 - k*91.5
k = 1.661*10^-3 min M/min
Given:
k = 1.661*10^-3 M/min
use relation between rate constant and half life of 0 order reaction
t1/2 = [A]o/(2*k)
= 0.544/(2*1.661*10^-3)
= 1.637*10^2 min
Answer: 164 min
Only 1 question at a time please
Consider the following reaction. Calculate the value of the rate constant.. 2 A + B →→ 2 C A B C Rate Trial 1: 0.64 0.56 0.012 7.463 Trial 2: 1.28 0.56 0.012 14.926 Trial 3: 0.64 1.12 0.012 14.926 Trial 4: 0.1 0.4 0.012 ?
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