At a certain temperature this reaction follows first-order kinetics with a rate constant of Suppose a vessel contains at a concentration of . Calculate the concentration of in the vessel seconds later. You may assume no other reaction is important. Round your answer to significant digits.

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.

0.41 M

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

it is stable as it is in group 0 which have full outer shells of electrons