Lena772
  • Lena772
A reaction has a rate law of : rate = k [ClO3-] [Cl-] [H+]2. If the initial reaction rate is 3.2E-3 M/s, then what is the rate constant if the initial concentrations are [ClO3-]o= 0.10 M, [Cl-]o= 0.10 M, [H+]o= 0.20 M ? (units are M-3 " s-1) A) 1.6 B) 8.0 C) 1.2 D) 0.62 E) none of these
Chemistry
chestercat
  • chestercat
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Lena772
  • Lena772
Abhisar
  • Abhisar
Ok, so have you tried it first urself?
Lena772
  • Lena772
i think you would say 3.2 E-3 M/s = k [0.10] [0.10] [0.2] k= (3.2E-3/([0.10]*[0.1)]*[0.20])

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Abhisar
  • Abhisar
Yes, that's correct c:
Lena772
  • Lena772
k= 0.064
Abhisar
  • Abhisar
Check for one thung!!!
Lena772
  • Lena772
so i guess D iis closest
Abhisar
  • Abhisar
No, you did a minor mistake !!!
Lena772
  • Lena772
actually wrong brackets... 1.6
Lena772
  • Lena772
A?
Abhisar
  • Abhisar
\(\sf Rate = k[ClO_3^-][Cl^-][H^+]^2\)
Abhisar
  • Abhisar
So, K should be equal to ???
Lena772
  • Lena772
1.6*0.10*0.20*0.10=3.2 E-3 (the initial rate) so k is 1.6
Lena772
  • Lena772
A :) thank you
Lena772
  • Lena772
That was incorrect :(
Abhisar
  • Abhisar
Nuuuuu!!! \(\sf K=\Large \frac{Rate}{[ClO_3^-][Cl^-][H^+]^2}\)
Abhisar
  • Abhisar
You need to keep the order as given, I said you did a mistake. look above.. :(
Lena772
  • Lena772
i got 1.6 when i calclulated that
Abhisar
  • Abhisar
It should be 8
Abhisar
  • Abhisar
\(\sf K=\Large \frac{3.2 \times 10^{-3}}{0.1\times 0.1 \times (0.2)^2}\)
Lena772
  • Lena772
why is 0.2 squared
Abhisar
  • Abhisar
Because the Rate Law is given as \(\sf Rate = k[ClO_3^-][Cl^-][H^+]^2\)
Lena772
  • Lena772
oh okay I didn't see that !
Abhisar
  • Abhisar
C;
Lena772
  • Lena772
thank you!

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