Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: serah1206 on February 27, 2019, 02:34:05 AM
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The question is to calculate the activation energy. I'm given this table
Expt Temp Time (s) [A] [ B ] [C] [D]
1 25 0 0.250 0.500 0 0
1.0 0.238 0.482 0.0060 0.0240
2 25 0 0.350 0.500 0 0
1.0 0.333 0.475 0.0085 0.0340
3 77 0 0.350 0.250 0 0
1.0 0.334 0.226 0.0080 0.0320
4 77 0 0.300 0.200 0 0
1.0 0.289 0.183 0.0055. 0.0220
I've determined the reaction rate is Rate = k [A]2 [ B ]3
I know I need to use the Arrhenius equation to find the activation energy, but I am confused as to what values to use to find my rate constant and what rates I should be using.
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I've determined the reaction rate is Rate = k [A]2 [ B ]3
How did you determine that? (Hint: it's wrong.)
Have you actually determined the stoichiometry of the reaction?
2A + 3B :rarrow: C + 4D
The order of a reaction is not necessarily related to the stoichiometry. A very important principle of kinetics.
How do you determine the order of the reaction with respect to a reagent?