Question

The rate law for a hypothetical reaction is
rate = k [A]^2. When the concentration is 0.10 moles/liter, the rate is 2.7 × 10^-5 M*s^-1. What is the value of k?

Answer 1

rate = k [A]^2
just plug in
2.7*10^(-5) = k*.1^2
^rate ^.1 molles/liter
maybe and then solve for k :)

Answer 2

k = 0.27e-2

Answer 3

umhm so wait...
would it be the same as
2.7*10^-3M^-1s^-1?

Answer 4

well unites should be

M*s^-1

so
( moles/liter)^2* k's units= M*s^-1

Answer 5

umhm alright. Thank you!

Answer 6

is
moles/liter=M?

Answer 7

remember the unit M=mol/L
\[
2.7\times10^{-5}\,{\rm M/s}=k\times \left(0.1\,{\rm M}\right)^2\\
k=\frac{2.7\times10^{-5}}{0.01}\times \frac{{\rm M}}{\rm s\cdot M^2}\\
\boxed{k=2.7\times10^{-3}{\rm M^{-1}\cdot s^{-1}}}
\]
the reaction is thus, a second order reaction.

Answer 8

Soo, I was right? :D
woho! Thanks alot electrokid!

Answer 9

yaya. good job.