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Rates of Reaction question.

  • Thread starter Saterial
  • Start date
  • #1
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Homework Statement


At 35C, the rate constant for the reaction: C12H22O11 + H20 --> C6H12O6 + C6H12O6 is k=6.2 x 10^-5 s-1. The activation energy for the reaction is 108 kJ/mol. What is the rate constant for the reaction at 45C? Determine the impact on the rate.


Homework Equations


r=Ae^-Ae/RT
r=k[C12H22O11][H2O]

The Attempt at a Solution



I don't know if I am even using the right equation, (Arrhenius equation) however I tried seperating the reaction into 35C and 45C stages and analyzed from there. At 35C, Ae is given so I plugged the Ae into the Arrhenius eq at 45C and cancel out the A base as it is the same at both 35C and 45C.

Ended up with :
r=e^(-108000/8.314*10). (change in temp of 10C)

Does this make any sense or even work? If so, what does the second part of impact on the rate mean?

Thanks a bunch.
 

Answers and Replies

  • #2
Borek
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What you found is ratio of rates, not rate. Use data for 35 deg C to find A, then just plug and chug for 45 deg C.
 
  • #3
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Also, given that the constant is given by J/Mol K, I would have thought you were supposed to use Kelvins instead of degrees Celsius.
 
  • #4
Borek
Mentor
28,404
2,802
When it comes to delta T it doesn't matter. A lot depends on how Saterial got to the expression shown.
 
  • #5
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When it comes to delta T it doesn't matter. A lot depends on how Saterial got to the expression shown.
Ah. Missed we were using delta.
 

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