Reaction Mechanisms or rate constants
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Reaction Mechanisms or rate constants
How can the Arrhenius equation be modified to account for non-Arrhenius behavior, such as temperature-dependent changes in reaction mechanism or rate constants?
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Re: Reaction Mechanisms or rate constants
The Arrhenius equation is sometimes expressed as k = Ae-E/RT where k is the rate of chemical reaction, A is a constant depending on the chemicals involved, E is the activation energy, R is the universal gas constant, and T is the temperature.
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Re: Reaction Mechanisms or rate constants
Hi!
The Arrhenius Equation can be used to determine the activation energy, temperature, and reaction rate.
Cooling slows down the reaction, and when reactants collide, higher temperature results in more collision. (Temperature increases and K increases).
Reactants must collide with enough energy to break bonds: Activation energy increases and K decreases. The activation is the energy barrier.
I hope this helps :)
The Arrhenius Equation can be used to determine the activation energy, temperature, and reaction rate.
Cooling slows down the reaction, and when reactants collide, higher temperature results in more collision. (Temperature increases and K increases).
Reactants must collide with enough energy to break bonds: Activation energy increases and K decreases. The activation is the energy barrier.
I hope this helps :)
Re: Reaction Mechanisms or rate constants
One approach is to introduce a temperature-dependent the pre-exponential or frequency factor into the equation. This factor accounts for changes in the frequency of collisions between reactant molecules due to changes in temperature.
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