Consider the exothermic reaction between nitrogen monoxide and ozone to form nitrogen dioxide and diatomic oxygen. a. Write and balance a chemical equation. b. Convert the chemical... Consider the exothermic reaction between nitrogen monoxide and ozone to form nitrogen dioxide and diatomic oxygen. a. Write and balance a chemical equation. b. Convert the chemical equation into a particle view of the molecules. c. Sketch an energy profile for the reaction, and use particle views to label the reactants and products. Show the effect a catalyst might have on the energy profile. d. Draw a possible transition state for the bimolecular reaction. Use dashed lines to represent the bonds that break and those that form.
Understand the Problem
The question describes an exothermic reaction between nitrogen monoxide (or nitric oxide) and ozone. It requires you to: (a) write a balanced chemical equation for the reaction, (b) represent the reaction using a particle view of the molecules, (c) sketch an energy profile diagram including the effect of a catalyst, and (d) draw a possible transition state showing bond breaking and bond forming.
Answer
a. NO(g) + O3(g) → NO2(g) + O2(g) b. Particle view: NO + O3 → NO2 + O2 c. Exothermic energy profile with catalyst lowering activation energy. d. Transition state: N-O bond forming, O-O bond breaking (dashed lines).
a. NO(g) + O3(g) → NO2(g) + O2(g) b. A particle view would show one molecule of NO reacting with one molecule of O3 to produce one molecule of NO2 and one molecule of O2. c. An energy profile would show reactants (NO + O3) at a higher energy level than the products (NO2 + O2), indicating an exothermic reaction. The peak of the curve represents the activation energy. A catalyst lowers this peak. d. The transition state would show the N-O bond forming between NO and O3, and an O-O bond breaking in O3, represented by dashed lines.
Answer for screen readers
a. NO(g) + O3(g) → NO2(g) + O2(g) b. A particle view would show one molecule of NO reacting with one molecule of O3 to produce one molecule of NO2 and one molecule of O2. c. An energy profile would show reactants (NO + O3) at a higher energy level than the products (NO2 + O2), indicating an exothermic reaction. The peak of the curve represents the activation energy. A catalyst lowers this peak. d. The transition state would show the N-O bond forming between NO and O3, and an O-O bond breaking in O3, represented by dashed lines.
More Information
This reaction is important in atmospheric chemistry, particularly regarding the ozone layer. Nitrogen monoxide (NO) can catalyze the destruction of ozone (O3), contributing to ozone depletion. The transition state is a critical concept in understanding reaction mechanisms.
Tips
A common mistake is not balancing the chemical equation correctly. Also, the energy profile should clearly show that the products are at a lower energy level than the reactants for an exothermic reaction. When drawing the transition state, remember to use dashed lines to represent bonds forming and breaking.
Sources
AI-generated content may contain errors. Please verify critical information
