The first-order decomposition of n2o at 1000 k has a rate constant of 0.76 s-1. if the initial concentration of n2o is 10.9 m, what is the concentration of n2o after 9.6 s

For a first-order reaction, the rate law would be expressed as:

r = dC / dt = - kC

Integrating it from time zero and the initial concentration, Co, to time, t, and the final concentration, C. We will obtain the first-order integrated law as follows:

ln C/Co = - kt

To determine the concentration of N2O in the system at a certain time, we simply substitute the given values from the problem statement as follows:

ln C / Co = - kt

ln C / 10.9 = - 0.76 (9.6)

e^ln C / 10.9 = e^-0.76 (9.6)

C / 10.9 = 6.78 x 10^-4

C = 7.39 x 10^-3 m

Therefore, the concentration of N2O in the system after 9.6 s would be 7.39 x10^-3 m.