If the initial concentration of NONO is 0.175 MM, what is the equilibrium concentration of N2N2?

Given that the initial concentration of NO is 0.175 M and using the previous analysis, we can determine the equilibrium concentration of \(\text{N}_2\) based on the reaction:

\[
2 \text{NO}(g) \rightleftharpoons \text{N}_2(g) + \text{O}_2(g)
\]

From the ICE table set up earlier:

| Species        | Initial (M)       | Change (M)        | Equilibrium (M) |
|----------------|-------------------|-------------------|-----------------|
| \(\text{NO}\)  | 0.175             | \(-2x\)            | \(0.175 - 2x\)  |
| \(\text{N}_2\) | 0                 | \(+x\)             | \(x\)           |
| \(\text{O}_2\) | 0                 | \(+x\)             | \(x\)           |

We calculated earlier that \(x\), the change in concentration, is approximately \(0.0866 \, M\).

### Equilibrium concentration of \( \text{N}_2 \):

\[
[\text{N}_2]_{eq} = x = 0.0866 \, M
\]

So, the equilibrium concentration of \(\text{N}_2\) is approximately \(0.0866 \, M\).

Do you want further explanation or have any other questions?

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Here are some related questions to consider:

1. How would the equilibrium concentration of \(\text{N}_2\) change if the initial concentration of NO were increased?
2. What is the effect of temperature on the equilibrium concentration of \(\text{N}_2\)?
3. How can you calculate the partial pressure of \(\text{N}_2\) at equilibrium?
4. What is the relationship between the equilibrium constant \(K_c\) and the concentrations of reactants and products?
5. How does the stoichiometry of the reaction affect the equilibrium concentrations?
6. What would happen to the equilibrium concentration of \(\text{N}_2\) if the volume of the system is decreased?
7. How would the equilibrium position change if a catalyst is added to the reaction?
8. Can the equilibrium concentration of \(\text{N}_2\) be directly measured experimentally?

**Tip:** When dealing with equilibrium problems, carefully track the stoichiometric coefficients since they directly influence how concentration changes relate to each other.

Understand how to calculate the equilibrium concentration of N2 from the initial concentration of NO using chemical equilibrium principles. This problem involves setting up an ICE table and applying stoichiometric relationships to determine the equilibrium concentration of N2. Suitable for advanced high school and college chemistry students.

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