The following information was obtained for the rate constant, k, for a reaction at 25 OC
A
|
Ea
|
R
|
2.57 × 109 s–1
|
96.2 kJ mol–1
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8.31 J K–1 mol–1
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Which expression correctly represents how to calculate the rate constant, k?
k = (2.57 x 109) x e(-96.2 / 8.31×25)
k = (2.57 x 109) x e(-96.2 / 8.31×298)
k = (2.57 x 109) x e(-96200 / 8.31×25)
k = (2.57 x 109) x e(-96200 / 8.31×298)
The following experimental data was collected.
Activation energy, Ea
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111 kJ mol–1
|
Rate constant, k
|
1.30 x 10-4 mol-1 dm3 s-1
|
Arrhenius constant, A
|
4.55 × 1013 mol-1 dm3 s-1
|
Which expression correctly calculates the temperature of the reaction?
Consider the following statements:
- Many reactions show a doubling of the rate with a temperature increase of 10K
- The units of k for a second order reaction are mol-1 dm3 s-1
- In the Arrhenius equation, A relates to the energy requirements of the collisions
Which statements are correct?