For the elementary process N2 O5(g) ⟶NO2(g)+NO3(g) the activation energy (Ea) and overall ΔE are

step 1 Chapter 14, question 56. For the elementary process, the activation energy and overall delta E a

For the elementary process N2 O5(g) ⟶NO2(g)+NO3(g) the...

For the elementary process $\mathrm{N}_{2} \mathrm{O}_{5}(g) \longrightarrow \mathrm{NO}_{2}(g)+\mathrm{NO}_{3}(g)$ the activation energy $\left(E_{a}\right)$ and overall $\Delta E$ are 154 $\mathrm{kJ} / \mathrm{mol}$ and 136 $\mathrm{kJ} / \mathrm{mol}$ , respectively. (a) Sketch the energy profile for this reaction, and label $E_{a}$ and $\Delta E$ . (b) What is the activation energy for the reverse reaction?

Key Concepts

Forward and Reverse Reaction Energetics

The energetics of forward and reverse reactions are interrelated through the reaction’s overall energy change. For an elementary reaction, the activation energy for the reverse reaction can be determined by subtracting the overall energy change (?E) from the forward activation energy, highlighting how the thermodynamic energy difference impacts the kinetic barrier in the reverse process.

Elementary Reaction

An elementary reaction is a single-step process characterized by a specific molecularity, meaning the reaction occurs in one elementary event. In such reactions, the rate law can be directly deduced from the stoichiometry because the reaction proceeds through a single transition state without intermediates.

Energy Profile Diagram

An energy profile diagram, or reaction coordinate diagram, visually represents the progress of a reaction in terms of energy changes. It typically shows the energy levels of the reactants, products, and transition state, allowing one to identify both the activation energy and the overall energy change of the reaction.

Activation Energy

Activation energy is the minimum energy needed for reactants to transform into products. It represents the energy barrier that must be overcome for a reaction to proceed and is key for understanding reaction kinetics and the rates at which reactions occur.

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