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.

0.57 M

Explanation:

rate = change in concentration / time

Initial concentration of Cl2O5 = 1.16 M

Let the concentration of Cl2O5 after 5.70 seconds be y

rate = (1.16 - y) / 5.7

The reaction follows a first order

Therefore, rate = ky = 0.184y

0.184y = (1.16 - y) / 5.7

0.184y * 5.7 = 1.16 - y

1.0488y + y = 1.16

2.0488y = 1.16

y = 1.16/2.0488 = 0.57 M

Concentration of Cl2O5 after 5.70 seconds is 0.57 M