We’re given the following first order reaction:
A → B k = 0.83 min–1
The integrated rate law for a first order reaction is as follows:
where [A]t = concentration at time t, k = rate constant, t = time, [A]0 = initial concentration.
We’re being asked to calculate the amount of A after 15 mins if we start with 3.6 M A.
This means we have:
[A]0 = 3.6 M k = 0.83 min–1
[A]t = ? t = 15 min
The reaction A → B follows first order kinetics with k = 0.83 min–1. If the initial concentration of A is 3.6 M, what is the concentration of A after 15 minutes?
A. 0.046 M
B. 0.230 M
C. 1.1×10–1 M
D. 1.84×10–3 M
E. 1.4×10–5 M
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