Review I Constants I Periodic Table Phosgene (carbonyl chloride), COClą, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at hi temperatures: CO(g) + Cl₂ (g) COC12 (g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 453 °C. At equilibrium, the concentrations were measured and the following results obtained: What is the equilibrium constant, Kp, of this reaction? Express your answer numerically. View Available Hint(s) Kp = Submit VE ΑΣΦ Part B 4 ? The following reaction was performed in a sealed vessel at 734 °C: D Gas Deriving concentrations from data In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K. CO Cl₂ COCI Partial Pressure (atm) 0.790 1.28 0.180 H₂(g) + 12(g) 2HI(g) Initially, only H₂ and I were present at concentrations of [H₂] = 3.75 M and [1₂] = 2.80M. The equilibrium concentration of I₂ is 0.0900 M. What is the equilibrium constant, Ke, for the reaction at this temperature? Express your answer numerically. View Available Hint(s)
Review I Constants I Periodic Table Phosgene (carbonyl chloride), COClą, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at hi temperatures: CO(g) + Cl₂ (g) COC12 (g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 453 °C. At equilibrium, the concentrations were measured and the following results obtained: What is the equilibrium constant, Kp, of this reaction? Express your answer numerically. View Available Hint(s) Kp = Submit VE ΑΣΦ Part B 4 ? The following reaction was performed in a sealed vessel at 734 °C: D Gas Deriving concentrations from data In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K. CO Cl₂ COCI Partial Pressure (atm) 0.790 1.28 0.180 H₂(g) + 12(g) 2HI(g) Initially, only H₂ and I were present at concentrations of [H₂] = 3.75 M and [1₂] = 2.80M. The equilibrium concentration of I₂ is 0.0900 M. What is the equilibrium constant, Ke, for the reaction at this temperature? Express your answer numerically. View Available Hint(s)
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![## Equilibrium Constant and Reaction Data Analysis
**Overview:**
Phosgene (carbonyl chloride), COCl₂, is an extremely toxic gas used in manufacturing dyes and plastics. It can be produced by reacting carbon monoxide and chlorine gas at high temperatures.
### Reaction:
\[ \text{CO}(g) + \text{Cl}_2(g) \rightleftharpoons \text{COCl}_2(g) \]
Carbon monoxide and chlorine gas were allowed to react in a sealed vessel at 453°C. At equilibrium, the concentrations were measured with the following results:
**Table of Partial Pressures:**
| Gas | Partial Pressure (atm) |
|---------|------------------------|
| CO | 0.790 |
| Cl₂ | 1.28 |
| COCl₂ | 0.180 |
**Question:**
What is the equilibrium constant, \( K_p \), of this reaction?
Express your answer numerically.
\[ K_p = \] [Text box for answer input]
**Submit Button**
---
**Deriving Concentrations from Data:**
In Part A, you were given equilibrium pressures to input directly into the formula for \( K \). In Part B, however, you will be given initial concentrations and only one equilibrium concentration. Derive all three equilibrium concentrations before applying the formula for \( K \).
### Part B:
The following reaction was performed in a sealed vessel at 734°C:
\[ \text{H}_2(g) + \text{I}_2(g) \rightleftharpoons 2\text{HI}(g) \]
Initially, only \(\text{H}_2\) and \(\text{I}_2\) were present at concentrations of \([\text{H}_2] = 3.75\,M\) and \([\text{I}_2] = 2.80\,M\). The equilibrium concentration of \(\text{I}_2\) is \(0.0900\,M\). What is the equilibrium constant, \( K_c \), for this reaction at this temperature?
Express your answer numerically.
\[ K_c = \] [Text box for answer input]
**Resources:**
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Transcribed Image Text:## Equilibrium Constant and Reaction Data Analysis
**Overview:**
Phosgene (carbonyl chloride), COCl₂, is an extremely toxic gas used in manufacturing dyes and plastics. It can be produced by reacting carbon monoxide and chlorine gas at high temperatures.
### Reaction:
\[ \text{CO}(g) + \text{Cl}_2(g) \rightleftharpoons \text{COCl}_2(g) \]
Carbon monoxide and chlorine gas were allowed to react in a sealed vessel at 453°C. At equilibrium, the concentrations were measured with the following results:
**Table of Partial Pressures:**
| Gas | Partial Pressure (atm) |
|---------|------------------------|
| CO | 0.790 |
| Cl₂ | 1.28 |
| COCl₂ | 0.180 |
**Question:**
What is the equilibrium constant, \( K_p \), of this reaction?
Express your answer numerically.
\[ K_p = \] [Text box for answer input]
**Submit Button**
---
**Deriving Concentrations from Data:**
In Part A, you were given equilibrium pressures to input directly into the formula for \( K \). In Part B, however, you will be given initial concentrations and only one equilibrium concentration. Derive all three equilibrium concentrations before applying the formula for \( K \).
### Part B:
The following reaction was performed in a sealed vessel at 734°C:
\[ \text{H}_2(g) + \text{I}_2(g) \rightleftharpoons 2\text{HI}(g) \]
Initially, only \(\text{H}_2\) and \(\text{I}_2\) were present at concentrations of \([\text{H}_2] = 3.75\,M\) and \([\text{I}_2] = 2.80\,M\). The equilibrium concentration of \(\text{I}_2\) is \(0.0900\,M\). What is the equilibrium constant, \( K_c \), for this reaction at this temperature?
Express your answer numerically.
\[ K_c = \] [Text box for answer input]
**Resources:**
- View Available Hint(s)
**Submit Button**
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