A
amarillo
Guest
The question goes:
For the first order decomposition of acetone at 650 K, the concentration of acetone was 0.350 M after 27.0 min and 0.191 M after 44 min.
I tried using the integrated rate law:
ln[A] = -kt + ln [A]0 (where [A]0 is my original concentration)
for a first order reaction, using 0.350M as my original concentration and 0.191 M as my other concentration. I ended up with k=9.38 x 10^-4 which was wrong.
Can someone please help?
For the first order decomposition of acetone at 650 K, the concentration of acetone was 0.350 M after 27.0 min and 0.191 M after 44 min.
I tried using the integrated rate law:
ln[A] = -kt + ln [A]0 (where [A]0 is my original concentration)
for a first order reaction, using 0.350M as my original concentration and 0.191 M as my other concentration. I ended up with k=9.38 x 10^-4 which was wrong.
Can someone please help?