4. For the reaction below: 2 NO2 (g) + O2 (g) 2 NO3 (g) a. Write the law of mass action (the equilibrium expression for Keq) Keq [NO312 [0₂] [NO₂]² Keq b. If gas concentrations are as follows, 2.10 M NO2, 1.75 M O2, and 1.00 M NO3, calculate Keq = 0.130 M-¹ (NOTE: "M-¹" is another way to write "1/M") [1.00 M12 [1.75 M ] [2.10 M]² c. Based on the Keq value that you calculated in part b, are the reactants or products predominant (predominant means that there is a greater amount present)? REACTANTS: Keq is much less than 1

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### Equilibrium Calculation for the Reaction

For the reaction:
\[ 2 \text{NO}_2 \, (g) + \text{O}_2 \, (g) \rightleftharpoons 2 \text{NO}_3 \, (g) \]

#### a. Law of Mass Action

Write the equilibrium expression, \( K_{eq} \), for the reaction:
\[ K_{eq} = \frac{[\text{NO}_3]^2}{[\text{O}_2][\text{NO}_2]^2} \]

#### b. Calculate \( K_{eq} \)

Given the concentrations:
- \([\text{NO}_2] = 2.10 \, \text{M}\)
- \([\text{O}_2] = 1.75 \, \text{M}\)
- \([\text{NO}_3] = 1.00 \, \text{M}\)

Substitute these values into the equation:
\[ K_{eq} = \frac{[1.00 \, \text{M}]^2}{[1.75 \, \text{M}][2.10 \, \text{M}]^2} = 0.130 \, \text{M}^{-1} \]

**Note:** "M\(^{-1}\)" means \( \frac{1}{\text{M}} \).

#### c. Predominance of Reactants or Products

Based on the \( K_{eq} \) value calculated (0.130 M\(^{-1}\)), determine the predominance of reactants or products. Since \( K_{eq} \) is much less than 1, the **reactants** are predominant in this equilibrium system.
Transcribed Image Text:### Equilibrium Calculation for the Reaction For the reaction: \[ 2 \text{NO}_2 \, (g) + \text{O}_2 \, (g) \rightleftharpoons 2 \text{NO}_3 \, (g) \] #### a. Law of Mass Action Write the equilibrium expression, \( K_{eq} \), for the reaction: \[ K_{eq} = \frac{[\text{NO}_3]^2}{[\text{O}_2][\text{NO}_2]^2} \] #### b. Calculate \( K_{eq} \) Given the concentrations: - \([\text{NO}_2] = 2.10 \, \text{M}\) - \([\text{O}_2] = 1.75 \, \text{M}\) - \([\text{NO}_3] = 1.00 \, \text{M}\) Substitute these values into the equation: \[ K_{eq} = \frac{[1.00 \, \text{M}]^2}{[1.75 \, \text{M}][2.10 \, \text{M}]^2} = 0.130 \, \text{M}^{-1} \] **Note:** "M\(^{-1}\)" means \( \frac{1}{\text{M}} \). #### c. Predominance of Reactants or Products Based on the \( K_{eq} \) value calculated (0.130 M\(^{-1}\)), determine the predominance of reactants or products. Since \( K_{eq} \) is much less than 1, the **reactants** are predominant in this equilibrium system.
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2NO2 (g) + O2 (g)   2NO3 (g)

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