The question is incomplete, the complete question is;
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.184 s^-1 ? Suppose a vessel contains Cl_2 O_5 at a concentration of 1.16 M. Calculate the concentration of Cl_2 O_5 in the vessel 5.70 seconds later. You may assume no other reaction is important.
Answer:
0.41 M
Step-by-step explanation:
Recall that for a first order reaction;
kt = ln [Ao]/[A]
Where;
k = rate constant = 0.184 s^-1
t=time elapsed = 5.70 seconds
[Ao] = initial concentration = 1.16 M
[A]= concentration at time t = the unknown
So,
e^kt = e^ln[Ao]/[A]
e^kt =[Ao]/[A]
[A] = [Ao]/e^kt
[A] = 1.16 M/e^(0.184s-1 * 5.70 s)
[A] = 0.41 M