- 3. Using this data, calculate a value for Kc for the reaction, A. 2.06 x 104 B. 4.84 x 10-3 C. 0.223 D. 4.49 E. 20.2 2 NO(g) + Cl₂(g) 2 NOCI(g) Kc = 3.20 x 10-3 2 NO2(g) 2 NO(g) + O₂(g) Kc = 15.5 NO2(g) + ½ Cl₂(g) 4. Using the data, NOCI(g) + 1/2O2(g) A3B4 (g) 2 AB (g) + AB2 (g) (g) 3 A (g) + 4 B (g) A3B4 (g) calculate a value for Kc for the reaction, 3 A (g) + 4 B Kc = 25 Kc = 3.75 2 AB (g) + AB2 (g)

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**Question 3: Using this data,**

\[ 2 \text{NO} (g) + \text{Cl}_2 (g) \rightleftharpoons 2 \text{NOCl} (g) \quad K_c = 3.20 \times 10^{-3} \]

\[ 2 \text{NO}_2 (g) \rightleftharpoons 2 \text{NO} (g) + \text{O}_2 (g) \quad K_c = 15.5 \]

Calculate a value for \( K_c \) for the reaction,

\[ \text{NOCl} (g) + \frac{1}{2} \text{O}_2 (g) \rightleftharpoons \text{NO}_2 (g) + \frac{1}{2} \text{Cl}_2 (g) \]

Options:
A. \( 2.06 \times 10^{-4} \)  
B. \( 4.84 \times 10^{-3} \)  
C. \( 0.223 \)  
D. \( 4.49 \)  
E. \( 20.2 \)  

**Question 4: Using the data,**

\[ 3 \text{A} (g) + 4 \text{B} (g) \rightleftharpoons \text{A}_3\text{B}_4 (g) \quad K_c = 25 \]

\[ \text{A}_3\text{B}_4 (g) \rightleftharpoons 2 \text{AB} (g) + \text{AB}_2 (g) \quad K_c = 3.75 \]

Calculate a value for \( K_c \) for the reaction,

\[ 3 \text{A} (g) + 4 \text{B} \rightleftharpoons 2 \text{AB} (g) + \text{AB}_2 (g) \]

---

This content provides information on how to calculate equilibrium constants (\( K_c \)) for given chemical reactions using known \( K_c \) values from related reactions. Understanding these principles is fundamental in chemistry, especially in the study of reaction dynamics and equilibria.
Transcribed Image Text:**Question 3: Using this data,** \[ 2 \text{NO} (g) + \text{Cl}_2 (g) \rightleftharpoons 2 \text{NOCl} (g) \quad K_c = 3.20 \times 10^{-3} \] \[ 2 \text{NO}_2 (g) \rightleftharpoons 2 \text{NO} (g) + \text{O}_2 (g) \quad K_c = 15.5 \] Calculate a value for \( K_c \) for the reaction, \[ \text{NOCl} (g) + \frac{1}{2} \text{O}_2 (g) \rightleftharpoons \text{NO}_2 (g) + \frac{1}{2} \text{Cl}_2 (g) \] Options: A. \( 2.06 \times 10^{-4} \) B. \( 4.84 \times 10^{-3} \) C. \( 0.223 \) D. \( 4.49 \) E. \( 20.2 \) **Question 4: Using the data,** \[ 3 \text{A} (g) + 4 \text{B} (g) \rightleftharpoons \text{A}_3\text{B}_4 (g) \quad K_c = 25 \] \[ \text{A}_3\text{B}_4 (g) \rightleftharpoons 2 \text{AB} (g) + \text{AB}_2 (g) \quad K_c = 3.75 \] Calculate a value for \( K_c \) for the reaction, \[ 3 \text{A} (g) + 4 \text{B} \rightleftharpoons 2 \text{AB} (g) + \text{AB}_2 (g) \] --- This content provides information on how to calculate equilibrium constants (\( K_c \)) for given chemical reactions using known \( K_c \) values from related reactions. Understanding these principles is fundamental in chemistry, especially in the study of reaction dynamics and equilibria.
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