anonymous
  • anonymous
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?
Chemistry
schrodinger
  • schrodinger
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anonymous
  • anonymous
rate = k [A]^2 just plug in 2.7*10^(-5) = k*.1^2 ^rate ^.1 molles/liter maybe and then solve for k :)
anonymous
  • anonymous
k = 0.27e-2
anonymous
  • anonymous
umhm so wait... would it be the same as 2.7*10^-3M^-1s^-1?

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anonymous
  • anonymous
well unites should be M*s^-1 so ( moles/liter)^2* k's units= M*s^-1
anonymous
  • anonymous
umhm alright. Thank you!
anonymous
  • anonymous
is moles/liter=M?
anonymous
  • anonymous
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.
anonymous
  • anonymous
Soo, I was right? :D woho! Thanks alot electrokid!
anonymous
  • anonymous
yaya. good job.

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