In the problem, we are asked to find which of the two plots has a larger value for the activation energy (EA).
The Arrhenius Equation shows the dependence of the rate constant on the pre-exponential factor, absolute temperature and activation energy of the reaction.
Mathematically, the Arrhenius Equation is expressed as:
k is the rate constant
A is the frequency factor
Ea is the activation energy
R is the gas constant (8.314 J/mol•K )
T is the temperature
To solve this problem we must relate the Arrhenius Equation to the plot of the graph.
The accompanying graph shows plots of ln k versus 1/T for two different reactions. The plots have been extrapolated to the y-intercepts.
Which reaction has the larger value for Ea?
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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 Zellmer's class at OSU.