Question

According to the Arrhenius equation ______.

पर्याय

• a high activation energy usually implies a fast reaction.

• rate constant increases with increase in temperature. This is due to a greater number of collisions whose energy exceeds the activation energy.

• higher the magnitude of activation energy, stronger is the temperature dependence of the rate constant.

• the pre-exponential factor is a measure of the rate at which collisions occur, irrespective of their energy.

Answer 1

According to the Arrhenius equation rate constant increases with increase in temperature. This is due to a greater number of collisions whose energy exceeds the activation energy, higher the magnitude of activation energy, stronger is the temperature dependence of the rate constant and the pre-exponential factor is a measure of the rate at which collisions occur, irrespective of their energy.

Explanation:

according to Arrhenius equation:

\[\ce{k = Ae^{-E_a/RT}}\]

When \[\ce{T -> \infty}\] then \[\ce{e^{-E_a/RT} -> 0}\] which means that \[\ce{k -> A}\], Then we can observe that as the temperature rises, so does the rate constant, which approaches the Arrhenius constant. As we all know, increased activation energy reduces the rate of reaction, whereas higher temperature increases it. As a result, at higher activation energies, or when the activation energy is constant, the rate of reaction is not affected by temperature. The pre-exponential factor is always constant for a given reaction, regardless of temperature. It denotes the frequency of contact at a standard concentration.