An 1.00-L flask containing 8.53 g of SO2 Cl2 is heated to 375 °C. What is the concentration of SO₂ Cl₂ in the system when equilibrium is achieved? Concentration = mol/L

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Chapter1: Chemical Foundations
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Sulfury chloride, \( \text{SO}_2\text{Cl}_2 \), is a compound with very irritating vapors; it is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature, it decomposes to \( \text{SO}_2 \) and \( \text{Cl}_2 \).

\[
\text{SO}_2\text{Cl}_2 (g) \rightleftharpoons \text{SO}_2 (g) + \text{Cl}_2 (g) \quad K_c = 0.045 \text{ at } 375^\circ\text{C}
\]
Transcribed Image Text:Sulfury chloride, \( \text{SO}_2\text{Cl}_2 \), is a compound with very irritating vapors; it is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature, it decomposes to \( \text{SO}_2 \) and \( \text{Cl}_2 \). \[ \text{SO}_2\text{Cl}_2 (g) \rightleftharpoons \text{SO}_2 (g) + \text{Cl}_2 (g) \quad K_c = 0.045 \text{ at } 375^\circ\text{C} \]
**Chemical Equilibrium Problem**

A 1.00-L flask containing 8.53 grams of \( \text{SO}_2\text{Cl}_2 \) is heated to 375°C. What is the concentration of \( \text{SO}_2\text{Cl}_2 \) in the system when equilibrium is achieved?

Concentration = [ ] mol/L

*Note: The problem involves the calculation of the equilibrium concentration of sulfuryl chloride in a contained system where the substance is heated to a specific temperature.*
Transcribed Image Text:**Chemical Equilibrium Problem** A 1.00-L flask containing 8.53 grams of \( \text{SO}_2\text{Cl}_2 \) is heated to 375°C. What is the concentration of \( \text{SO}_2\text{Cl}_2 \) in the system when equilibrium is achieved? Concentration = [ ] mol/L *Note: The problem involves the calculation of the equilibrium concentration of sulfuryl chloride in a contained system where the substance is heated to a specific temperature.*
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