According to the Arrhenius equation,

According to the Arrhenius equation,
  1. A high activation energy usually implies a fast reaction
  2. Rate constant increase with increase in temperature. This is due to a greater number of collisions whose energy exceeds the activation energy
  3. Higher the magnitude of activation energy, stronger is the temperature dependence of the rate constant
  4. The pre-exponential factor is a measure of the rate at which collisions occur, irrespective of their energy.

Solution

A] k=Ae-Ea/RT
High Ea means less k, hence slower rate.
B] e-Ea/RT = fraction of molecules having kinetic energy greater than activation energy which increase as temperature increases.
C] ln k2k1=EaR1T1-1T2 i.e., ln K2k1∝Ea
D] Rate of reaction ∝ Total number of collisions × Fraction of collisions which can form product
Rate of reaction ∝ZAB×P×e-Ea/RT
∝A e-Ea/RT

Asked in: JEE Advanced 2016 (Paper 1)

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