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Noemi95
Group Title
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?
 one year ago
 one year ago
Noemi95 Group Title
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?
 one year ago
 one year ago

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timo86m Group TitleBest ResponseYou've already chosen the best response.0
rate = k [A]^2 just plug in 2.7*10^(5) = k*.1^2 ^rate ^.1 molles/liter maybe and then solve for k :)
 one year ago

timo86m Group TitleBest ResponseYou've already chosen the best response.0
k = 0.27e2
 one year ago

Noemi95 Group TitleBest ResponseYou've already chosen the best response.1
umhm so wait... would it be the same as 2.7*10^3M^1s^1?
 one year ago

timo86m Group TitleBest ResponseYou've already chosen the best response.0
well unites should be M*s^1 so ( moles/liter)^2* k's units= M*s^1
 one year ago

Noemi95 Group TitleBest ResponseYou've already chosen the best response.1
umhm alright. Thank you!
 one year ago

timo86m Group TitleBest ResponseYou've already chosen the best response.0
is moles/liter=M?
 one year ago

electrokid Group TitleBest ResponseYou've already chosen the best response.1
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.
 one year ago

Noemi95 Group TitleBest ResponseYou've already chosen the best response.1
Soo, I was right? :D woho! Thanks alot electrokid!
 one year ago

electrokid Group TitleBest ResponseYou've already chosen the best response.1
yaya. good job.
 one year ago
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