## concentration of first-order integrated rate law

$aR \to bP, Rate = -\frac{1}{a} \frac{d[R]}{dt} = \frac{1}{b}\frac{d[P]}{dt}$

Angela He 3B
Posts: 15
Joined: Fri Sep 25, 2015 3:00 am

### concentration of first-order integrated rate law

This is a textbook example and it seems super simple but i don't know what happened in the Self-test

"The rate law for the decomposition of 2N2O (g) -> 2N2 (g) + O2 (g) is Rate of decomposition of N2O = k[N2O]. Calculate the concentration of N2O remaining after the reaction has continued at 780 degrees Celsius for 100. ms, if the initial concentration of N2O is 0.20 mol/L and k = 3.4 s^(-1)."

I keep getting zero...

Laila Sathe 1D
Posts: 27
Joined: Fri Sep 25, 2015 3:00 am

### Re: concentration of first-order integrated rate law

Look at the units of the constants given (initial concentration and k) and the units that should be in your answer.