Assume that the following reaction is a single-step reaction...

Assume that the following reaction is a single-step reaction in which one of the $\mathrm{O}-\mathrm{O}$ bonds in $\mathrm{O}_3$ is broken and a new $\mathrm{N}-\mathrm{O}$ bond is formed. The heat of reaction is $-226 \mathrm{~kJ} / \mathrm{mol}$. $$ \mathrm{NO}(\mathrm{~g})+\mathrm{O}_3(\mathrm{~g}) \rightarrow \mathrm{NO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})+226 \mathrm{~kJ} $$ a. With reference to collision theory, describe the general process that takes place as this reaction moves from reactants to products. b. List the three requirements that must be met before a reaction between $\mathrm{NO}(\mathrm{g})$ and $\mathrm{O}_3(\mathrm{~g})$ is likely to take place. c. Explain why $\mathrm{NO}(\mathrm{g})$ and $\mathrm{O}_3(\mathrm{~g})$ must collide before a reaction can take place. d. Explain why it is usually necessary for the new N-O bonds to form at the same time as the $\mathrm{O}-\mathrm{O}$ bonds are broken. e. Draw a rough sketch of the activated complex. (You do not need to show bond angles. Be sure to show the bond that is breaking and the bond that is being formed.) f. Explain why a collision between $\mathrm{NO}(\mathrm{g})$ and $\mathrm{O}_3(\mathrm{~g})$ must have a certain minimum energy (activation energy) in order to proceed to products. g. The activation energy for this reaction is $132 \mathrm{~kJ} / \mathrm{mol}$. Draw an energy diagram for this reaction, showing the relative energies of the reactants, the activated complex, and the products. Using arrows show the activation energy and heat of reaction. h. Is this reaction exothermic or endothermic? i. Explain why $\mathrm{NO}(\mathrm{g})$ and $\mathrm{O}_3(\mathrm{~g})$ molecules must collide with the correct orientation if a reaction between them is going to be likely to take place.

Assume that the following reaction is a single-step reaction in which one of the $\mathrm{O}-\mathrm{O}$ bonds in $\mathrm{O}_3$ is broken and a new $\mathrm{N}-\mathrm{O}$ bond is formed. The heat of reaction is $-226 \mathrm{~kJ} / \mathrm{mol}$.

$$
\mathrm{NO}(\mathrm{~g})+\mathrm{O}_3(\mathrm{~g}) \rightarrow \mathrm{NO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})+226 \mathrm{~kJ}
$$

a. With reference to collision theory, describe the general process that takes place as this reaction moves from reactants to products.
b. List the three requirements that must be met before a reaction between $\mathrm{NO}(\mathrm{g})$ and $\mathrm{O}_3(\mathrm{~g})$ is likely to take place.
c. Explain why $\mathrm{NO}(\mathrm{g})$ and $\mathrm{O}_3(\mathrm{~g})$ must collide before a reaction can take place.
d. Explain why it is usually necessary for the new N-O bonds to form at the same time as the $\mathrm{O}-\mathrm{O}$ bonds are broken.
e. Draw a rough sketch of the activated complex. (You do not need to show bond angles. Be sure to show the bond that is breaking and the bond that is being formed.)
f. Explain why a collision between $\mathrm{NO}(\mathrm{g})$ and $\mathrm{O}_3(\mathrm{~g})$ must have a certain minimum energy (activation energy) in order to proceed to products.
g. The activation energy for this reaction is $132 \mathrm{~kJ} / \mathrm{mol}$. Draw an energy diagram for this reaction, showing the relative energies of the reactants, the activated complex, and the products. Using arrows show the activation energy and heat of reaction.
h. Is this reaction exothermic or endothermic?
i. Explain why $\mathrm{NO}(\mathrm{g})$ and $\mathrm{O}_3(\mathrm{~g})$ molecules must collide with the correct orientation if a reaction between them is going to be likely to take place.

Key Concepts

Exothermic Reactions

Exothermic reactions are reactions that release energy to their surroundings, typically in the form of heat. In these reactions, the products have lower energy than the reactants, which results in a net release of energy. This energy release is often depicted in energy diagrams and is a key signature of exothermic chemical processes.

Steric Factor (Orientation Requirement)

The steric factor refers to the need for proper alignment of molecules during collisions for a productive reaction to occur. Even if the colliding molecules have enough energy, they must also have the correct spatial orientation to allow for the efficient breaking of old bonds and the formation of new bonds, which is crucial for successful chemical reactions.

Energy Profile Diagram

An energy profile diagram is a graphical representation of the energy changes that occur during a chemical reaction. It shows the relative energies of the reactants, the activated complex (transition state), and the products. This diagram highlights both the activation energy required to initiate the reaction and, in exothermic reactions, the release of energy as the reaction proceeds to form lower-energy products.

Collision Theory

Collision theory explains that for a reaction to occur, reacting particles must collide with sufficient energy and proper orientation. It is a framework used to understand reaction rates by considering that molecules must physically come together to overcome an energy barrier, allowing bonds to break and new bonds to form.

Activation Energy

Activation energy is the minimum energy that colliding molecules must possess for a reaction to occur. It represents the energy barrier that must be overcome in order for the reactants to be transformed into products, and is typically illustrated as the difference in energy between the reactants and the highest energy state in the reaction pathway.

Activated Complex

The activated complex, or transition state, is a transient configuration of atoms at the peak of the energy barrier in a reaction. It is an unstable arrangement where old bonds are breaking and new bonds are forming simultaneously, representing the critical point at which the reaction can either proceed to form products or return to reactants.

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