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April 16, 2014

April 16, 2014

Posted by **m** on Tuesday, March 5, 2013 at 8:56pm.

The gas reaction N2O5 → 2NO2 + 1/2O2 follows the Arrhenius equation k = Ae(-Ea/RT) where R = 8.314 J K-1 mol-1 and 1 calorie = 4.184J. At the temperature T=273K, k = 3.46 x 10-5 s-1, whereas at T = 298K, k = 8.87 x 10-3 s-1. What is the value of the activation energy Ea in kJ/mol and in kcal/mol. What is the rate constant at 100 oC?

ln(3.46 x10-5 s-1)/(8.87 x 10-3 s-1)=Ea/(8.314 J/(K.mol))(1/(298 K)-1/273k)

Ea= 1.50 x 105 J or 150 kJ

- Chemistry -
**DrBob222**, Tuesday, March 5, 2013 at 10:00pm150 kJ is correct.

- Chemistry -
**m**, Tuesday, March 5, 2013 at 10:31pmI need to know the kcal/mol. How do I find the kcal/mol??

- Chemistry -
**DrBob222**, Tuesday, March 5, 2013 at 11:17pm1 cal = 4.184 J.

1 kcal = 4.184 kJ

- Chemistry -
**DrBob222**, Tuesday, March 5, 2013 at 11:48pm150 kJ is correct.

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