idk__21
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The rate constant, k, for a reaction varies with temperature as shown by the equation
k = Ae–EaIRT
For this reaction, at 25 °C, k = 3.46 × 10−8 s−1
The activation energy Ea = 96.2 kJ mol−1
The gas constant R = 8.31 J K−1 mol−1
Calculate a value for the Arrhenius constant, A, for this reaction.
Give the units for A

can someone show the working out for this question pls?
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Pigster
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(Original post by idk__21)
The rate constant, k, for a reaction varies with temperature as shown by the equation
k = Ae–EaIRT
For this reaction, at 25 °C, k = 3.46 × 10−8 s−1
The activation energy Ea = 96.2 kJ mol−1
The gas constant R = 8.31 J K−1 mol−1
Calculate a value for the Arrhenius constant, A, for this reaction.
Give the units for A

can someone show the working out for this question pls?
Take the natural log of both sides (which spec. do you do? Both forms of the equation are on our datasheet), this will allow you to rearrange the equation to make A the subject.

Units wise: looking at the version of the equation you have, e to the power of anything is unitless, hence k = A x unitless. Go figure.
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