The activation energy of a reaction is z...

The activation energy of a reaction is zero. The rate constant of the reaction

increases with increase of temperature

decreases with decrease of temperature

decreases with incrrease of temperature

in nearly independent of temperature

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Arrhenius studies the effect of temperature on the rate of a reaction and postulted that rate constant varies with temperature exponentially as k=Ae^(E_(a)//RT) . Thuis method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied. If the rate of reaction doubles for 10^(@)C rise of temperature form 290K to 300K, the activation energy of the reaction will be approximately :

OP TANDON-CHEMICAL KINETICS-OBJECTIVE QUESTIONS (LEVEL-A)

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Which one of the following is not a first order reaction?
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