Use Arrhenius equation and calculate the activation energy for a first-order reaction if its rate constant increases from 10 s–1 to 100 s–1 as the temperature increases from 300 to 330 K.
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The Arrhenius equation is k = Ae^(-Ea/RT), where A is the frequency or pre-exponential factor and e^(-Ea/RT) represents the fraction of collisions that have enough energy to overcome the activation barrier (i.e., have energy greater than or equal to the activation energy Ea) at temperature T.
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