Calculate AG for the reaction given below if the partial pressure of NO₂ is 0.220 atm and the partial pressure of N₂O4 is 0.428 atm. 2NO2(g) = N₂O4(8) AG 298 of this reaction is -5.40 kJ per mole of N₂O. T = 298K, R = 8.314 J.mol-¹.K-1 Note: Round you answer to 2 decimal places. AG = i kJ mol-1 Where does the system stand relative to equilibrium? O The system is at equilibrium, so that the reaction will not move. O The equilibrium shifts to products. O The equilibrium shifts to reactants.

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### Calculation of Gibbs Free Energy (\( \Delta G \))

**Problem Statement:**

Calculate \( \Delta G \) for the reaction given below if the partial pressure of \( \text{NO}_2 \) is 0.220 atm and the partial pressure of \( \text{N}_2\text{O}_4 \) is 0.428 atm.

\[ 2\text{NO}_2(\text{g}) \rightleftharpoons \text{N}_2\text{O}_4(\text{g}) \]

\( \Delta G^\circ_{298} \) of this reaction is -5.40 kJ per mole of \( \text{N}_2\text{O}_4 \).

**Given Constants:**

- Temperature (\( T \)) = 298 K
- Universal gas constant (\( R \)) = 8.314 J·mol\(^{-1}\)·K\(^{-1}\)

**Note:** Round your answer to 2 decimal places.

**Calculation Box:**

\[ \Delta G = \, \_\_\_\_\_ \, \text{kJ mol}^{-1} \]

### Equilibrium Consideration

**Question: Where does the system stand relative to equilibrium?**

**Options:**
- ○ The system is at equilibrium, so the reaction will not move.
- ○ The equilibrium shifts to products.
- ○ The equilibrium shifts to reactants.

This exercise asks learners to calculate the Gibbs Free Energy change (\( \Delta G \)) for the given reaction under specified conditions and predicts the direction of the equilibrium shift based on the calculated \( \Delta G \).
Transcribed Image Text:### Calculation of Gibbs Free Energy (\( \Delta G \)) **Problem Statement:** Calculate \( \Delta G \) for the reaction given below if the partial pressure of \( \text{NO}_2 \) is 0.220 atm and the partial pressure of \( \text{N}_2\text{O}_4 \) is 0.428 atm. \[ 2\text{NO}_2(\text{g}) \rightleftharpoons \text{N}_2\text{O}_4(\text{g}) \] \( \Delta G^\circ_{298} \) of this reaction is -5.40 kJ per mole of \( \text{N}_2\text{O}_4 \). **Given Constants:** - Temperature (\( T \)) = 298 K - Universal gas constant (\( R \)) = 8.314 J·mol\(^{-1}\)·K\(^{-1}\) **Note:** Round your answer to 2 decimal places. **Calculation Box:** \[ \Delta G = \, \_\_\_\_\_ \, \text{kJ mol}^{-1} \] ### Equilibrium Consideration **Question: Where does the system stand relative to equilibrium?** **Options:** - ○ The system is at equilibrium, so the reaction will not move. - ○ The equilibrium shifts to products. - ○ The equilibrium shifts to reactants. This exercise asks learners to calculate the Gibbs Free Energy change (\( \Delta G \)) for the given reaction under specified conditions and predicts the direction of the equilibrium shift based on the calculated \( \Delta G \).
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