1002X) 7. Phosgene is a potent chemical warfare agent that is now a agreement. It decomposes by the reaction COC1₂ (g) CO (g) + Cl₂ (g) Kc = 8 Calculate all species, when 0.100 mol of COCl2 was decomp 10.0 L flask.
1002X) 7. Phosgene is a potent chemical warfare agent that is now a agreement. It decomposes by the reaction COC1₂ (g) CO (g) + Cl₂ (g) Kc = 8 Calculate all species, when 0.100 mol of COCl2 was decomp 10.0 L flask.
Chemistry
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Chapter1: Chemical Foundations
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![**Phosgene Decomposition Reaction**
Phosgene is a potent chemical warfare agent that is now outlawed by international agreement. It decomposes by the reaction:
\[ \text{COCl}_2 \, (g) \rightleftharpoons \, \text{CO} \, (g) + \text{Cl}_2 \, (g) \]
The equilibrium constant (\( K_c \)) for this reaction at 360°C is \( 8.3 \times 10^{-4} \).
**Problem Statement:**
Calculate all species when 0.100 mol of COCl₂ was decomposed and reached equilibrium in a 10.0 L flask.
**Solution Overview:**
The reaction is analyzed for equilibrium concentrations using the provided \( K_c \) value. Initial concentrations, changes in concentrations due to equilibrium shift, and equilibrium concentrations are typically set up using an ICE table (Initial, Change, Equilibrium) approach.
**Notes:**
- The handwritten calculations seem to address setting up an equation based on the equilibrium constant expression and solving for the concentrations of each species at equilibrium. The expression could result in a quadratic equation solved for the change in concentration (usually denoted as 'x').](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3f4c86b2-1247-4388-bf18-f90827f5643c%2F61f649e1-76fc-48c7-af64-5a49c9e82bc2%2Fr1ldmo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Phosgene Decomposition Reaction**
Phosgene is a potent chemical warfare agent that is now outlawed by international agreement. It decomposes by the reaction:
\[ \text{COCl}_2 \, (g) \rightleftharpoons \, \text{CO} \, (g) + \text{Cl}_2 \, (g) \]
The equilibrium constant (\( K_c \)) for this reaction at 360°C is \( 8.3 \times 10^{-4} \).
**Problem Statement:**
Calculate all species when 0.100 mol of COCl₂ was decomposed and reached equilibrium in a 10.0 L flask.
**Solution Overview:**
The reaction is analyzed for equilibrium concentrations using the provided \( K_c \) value. Initial concentrations, changes in concentrations due to equilibrium shift, and equilibrium concentrations are typically set up using an ICE table (Initial, Change, Equilibrium) approach.
**Notes:**
- The handwritten calculations seem to address setting up an equation based on the equilibrium constant expression and solving for the concentrations of each species at equilibrium. The expression could result in a quadratic equation solved for the change in concentration (usually denoted as 'x').
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