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(3)
However, we have many A molecules present at a concentration , (molecule/dm3). Adding up the collisions of all the A molecules per unit volume, , then the number of collisions of all the A molecules with all B molecules per time per unit volume is

(4)

Where Sr is the collision cross section (Å)2. Substituting for Sr and UR



[molecules/time/volume] (5)

If we assume all collisions result in reactions then



[molecules/time/volume] (6)

Multiplying and dividing by Avogadrósnumber, NAvo, we can put our equation for the rate of reaction in terms of the number of moles/time/vol.



(7)
(8)

where A is the frequency factor



(9)

(10)



Calculate the frequency factor A for the reaction

at 273K.

Additional Information

Using the values in Table PRS.3A-1

Collision Radii

Hydrogen H H=2.74 Å/4 = 0.68Å = 0.68 x 10–10m



Oxygen O2 Å 1.55Å = 1.5 x 10–10m




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