Answer:
The time the reaction takes is 12.4s
Explanation:
A reaction that follows the rate law:
Rate =k[A] is order 1 and follows the equation:
Ln[A] = -kt + ln[A]₀
Where [A] is concentration of the reaction after time t: 0.0350M
k is rate constant = 0.15s⁻¹
t is time in seconds
[A]⁰ is initial concentration = 0.225M
Ln[0.0350] = -0.15s⁻¹*t + ln[0.225]
-1.86075 = -0.15s⁻¹*t
12.4s = t
The time the reaction takes is 12.4s
