Question

The rate constant $k_1$ of a reaction is found to be double that of rate constant $k_2$ of another reaction. The relationship between corresponding activation energies of the two reactions at the same temperature ($E_1$ and $E_2$) can be represented as:

Answer 1

Arrhenius equation:

• The definition of the Arrhenius equation is an expression that demonstrates the relationship between the reaction constant of a chemical reaction, the absolute temperature, and the factor $\mathrm{A}$, which stands for the pre-exponential component.
• It is the frequency of collisions between reactant particles.
• The Arrhenius equation is expressed as $k\mathit{=}A{e}^{\mathit{-}{\mathit{E}}_{\mathit{a}}\mathit{/}\mathit{R}\mathit{T}}$. As a result, the reaction's rate constant lowers as the activation energy rises.

Relationship between activation energy of the two temperatures:

• The pace at which a chemical reaction occurs is known as the reaction rate.
• It is discovered that the reaction's rate constant doubles, resulting in a ratio of two to one between the rate constants for the first and second reactions.
• It is discovered that one reaction's rate constant $\left(k_1\right)$ is twice as large as another reaction's rate constant $\left(k_2\right)$.

Therefore, it has lower activation energy than the second reaction $(E_{\mathit{1}}\mathit{<}{E}_{\mathit{2}}\mathit{)}$.