The rate constant for the first-order reaction below is 0.0476. If the reaction is begun with an initial concentration of A equal to 0.95 M, what is the concentration of A after 29.01 s?
ANSWER:
The first order reaction has the integratd order as:
k = 2.303/t log[A]o/[A]
k = rate constant , t = time = 29.01s , [A]o = initial concentration, [A] = concentration of reactant at time T
0.0476 = 2.303/ 29.01 log[0.95] / [A]
log[0.95] / [A] = 0.599
[0.95] / [A] = antilog(0.599)
[0.95] / [A] = 3.97
[A] = 0.23 M
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