Question

In the Arrhenius equation, \(k = Ae^{- Ea / RT}\), which factor corresponds to the fraction of molecules that have kinetic energy greater than activation energy ?

• A. \(e^{- Ea / RT}\)
• B. \(e^{- Ea / R}\)
• C. \(e^{- Ea / T}\)
• D. \(e^{- Ea}\)
• E. \(Ae^{- Ea / R}\)

Hint:

As temperature increases, \(e^{-E_a/(RT)}\) increases, hence rate constant increases.

Answer 1

The Correct Option is A

Step 1: Understanding the Concept:
Arrhenius equation: \(k = A e^{-E_a/(RT)}\). \(A\) is frequency factor, \(e^{-E_a/(RT)}\) is Boltzmann factor.

Step 2: Detailed Explanation:
The exponential term \(e^{-E_a/(RT)}\) represents the fraction of molecules with energy \(\geq E_a\). \(A\) accounts for collision frequency and orientation.

Step 3: Final Answer:
The fraction of molecules with KE$>$Ea is \(e^{-E_a/(RT)}\).