Question

given the particulate model which depicts the mechanism for the decomposition of \\(\text{no}_2\\), answer the following questions.

step 1:
step 2:

part 1 (1 point)
what is the chemical formula for the intermediate?

part 2 (1 point)
write a balanced equation for the overall chemical reaction. do not add states of matter.

Explanation:

Identify chemical species from the particulate model

Using the Reaction Mechanisms knowledge point

• Red spheres represent oxygen (\(\text{O}\)) atoms and blue spheres represent nitrogen (\(\text{N}\)) atoms.
• Step 1 reactants: One \(\text{NO}\) molecule (one blue, one red) and one \(\text{NO}_2\) molecule (one blue, two red).
• Step 1 transition/products: The model shows a collision forming a temporary association, which then decomposes into \(\text{NO}\) (one blue, one red) and \(\text{NO}_3\) (one blue, three red).
• Step 1 equation:

$$\text{NO} + \text{NO}_2 ightarrow \text{NO} + \text{NO}_3$$

Simplifying by removing the spectator \(\text{NO}\) molecule that remains unchanged:

$$\text{NO}_2 ightarrow \text{NO}_3 + \text{something?}$$

Let's re-examine the spheres in Step 1:

• Left: \(\text{NO}\) (blue-red) + \(\text{NO}_2\) (red-blue-red).
• Middle: They collide to form a transient state.
• Right: \(\text{NO}\) (blue-red) + \(\text{NO}_3\) (blue with three red spheres).
• Wait, let's count the atoms on the right of Step 1: one blue-red (\(\text{NO}\)) and one blue-three red (\(\text{NO}_3\)).
• Total atoms on left: 2 blue, 3 red.
• Total atoms on right: 2 blue, 4 red. This is unbalanced.
• Let's look closer at Step 1:
• Reactant 1: \(\text{NO}_2\) (one blue, two red).
• Reactant 2: \(\text{NO}_2\) (one blue, two red).
• Yes, both reactant molecules in Step 1 have one blue sphere and two red spheres. Thus, they are both \(\text{NO}_2\).
• Products of Step 1: One \(\text{NO}\) (one blue, one red) and one \(\text{NO}_3\) (one blue, three red).
• Balanced Step 1 equation:

$$\text{NO}_2 + \text{NO}_2 ightarrow \text{NO} + \text{NO}_3$$

• Step 2:
• Reactant: \(\text{NO}_3\) (one blue, three red).
• Products: \(\text{NO}\) (one blue, one red) + \(\text{O}_2\) (two red).
• Balanced Step 2 equation:

$$\text{NO}_3 ightarrow \text{NO} + \text{O}_2$$

Determine the chemical formula of the intermediate

Using the Reaction Intermediates knowledge point

• An intermediate is produced in an early step and consumed in a subsequent step.
• \(\text{NO}_3\) is produced in Step 1 and consumed in Step 2.
• Therefore, the intermediate is \(\text{NO}_3\).

Determine the overall balanced chemical equation

Using the Overall Reaction Equations knowledge point

• Sum the elementary steps:

$$
LATEXBLOCK0
$$

Answer:

Question 1

\(\text{NO}_3\)

Question 2

\(2\text{NO}_2
ightarrow 2\text{NO} + \text{O}_2\)