Questions: A reaction profile (not to scale) for the reaction NO + CO2 → NO2 + CO is shown below: Reaction Coordinate What is the value of the activation energy for this reaction? kJ Is this reaction exothermic or endothermic? What is the value of ΔE for the reaction? kJ

Transcript text: A reaction profile (not to scale) for the reaction \[ \mathrm{NO}+\mathrm{CO}_{2} \longrightarrow \mathrm{NO}_{2}+\mathrm{CO} \] is shown below: Reaction Coordinate What is the value of the activation energy for this reaction? $\square$ kJ Is this reaction exothermic or endothermic? $\square$ What is the value of $\Delta E$ for the reaction? $\square$ kJ

Solution

Solution Steps

Step 1: Determine the Activation Energy

The activation energy (Ea) is the energy difference between the reactants and the peak of the energy profile. From the graph, the energy of the reactants (NO + CO2) is at the baseline, and the peak is at 358 kJ.

Activation Energy (Ea) = 358 kJ

Step 2: Determine if the Reaction is Exothermic or Endothermic

To determine if the reaction is exothermic or endothermic, compare the energy of the reactants and the products. The energy of the products (NO2 + CO) is 226 kJ, which is lower than the energy of the reactants (baseline).

Since the products have lower energy than the reactants, the reaction releases energy and is therefore exothermic.

The reaction is exothermic.

Step 3: Calculate the Change in Energy (ΔE)

The change in energy (ΔE) is the difference between the energy of the products and the energy of the reactants.

ΔE = Energy of Products - Energy of Reactants ΔE = 226 kJ - 0 kJ ΔE = -132 kJ