Problem: The rate constant of a reaction is 4.50×10−5 L/mol•s at 195°C and 3.20 x 10-3 L/mol•s at 258°C. What is the activationenergy of the reaction?

FREE Expert Solution

We’re being asked to determine the activation energy (Ea) of a reaction. We’re given the rate constants at two different temperatures.


This means we need to use the two-point form of the Arrhenius Equation:

ln k2k1 = -EaR[1T2-1T1]



where 

k1 = rate constant at T1

k2 = rate constant at T2

Ea = activation energy (in J/mol)

R = gas constant (8.314 J/mol•K)

T1 and T2 = temperature (in K)


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Problem Details

The rate constant of a reaction is 4.50×10−5 L/mol•s at 195°C and 3.20 x 10-3 L/mol•s at 258°C. What is the activation
energy of the reaction?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Arrhenius Equation concept. You can view video lessons to learn Arrhenius Equation. Or if you need more Arrhenius Equation practice, you can also practice Arrhenius Equation practice problems.

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Based on our data, we think this problem is relevant for Professor Bertolini's class at USC.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.