Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Violet89 on February 24, 2013, 09:29:00 PM
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A first order reaction has an activation energy of 68.1 kJ/mol and a frequency factor (Arrhenius constant) of 1.48 x 1012 sec -1. Calculate the rate constant at 18°C.
K = A * exp(- Ea / RT)
I understand what to plug into this equation, but I keep getting the wrong answer. I calculate (- Ea / RT), press 2nd + LN, and multiply that by A. Am I doing something wrong?
I'd appreciate any help.
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Are you using R= 0.008314 KJK-1mol-1?
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Are you using R= 0.008314 KJK-1mol-1?
...or T=18, or a frequency factor of ~ 1500?
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I calculate (- Ea / RT), press 2nd + LN
On my TI that would mean calculating natural logarithm, not [itex]e^{\frac {-E_a} {RT}}[/itex].