Suppose a 250. mL flask is filled with 0.50 mol of Cl₂, 1.2 mol of CHCl3 and 0.80 mol of CC14. The following reaction becomes possible: Cl₂(g) + CHC1₂(g) → HC1(g) + CC1₂(g) The equilibrium constant K for this reaction is 5.15 at the temperature of the flask. Calculate the equilibrium molarity of HC1. Round your answer to two decimal places. X S ?
Suppose a 250. mL flask is filled with 0.50 mol of Cl₂, 1.2 mol of CHCl3 and 0.80 mol of CC14. The following reaction becomes possible: Cl₂(g) + CHC1₂(g) → HC1(g) + CC1₂(g) The equilibrium constant K for this reaction is 5.15 at the temperature of the flask. Calculate the equilibrium molarity of HC1. Round your answer to two decimal places. X S ?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Answer with two decimal places, please!
![**Chemistry Equilibrium Calculation Example:**
**Problem Statement:**
Suppose a 250 mL flask is filled with 0.50 mol of Cl₂, 1.2 mol of CHCl₃, and 0.80 mol of CCl₄. The following reaction becomes possible:
\[ \text{Cl}_2(\text{g}) + \text{CHCl}_3(\text{g}) \rightleftharpoons \text{HCl}(\text{g}) + \text{CCl}_4(\text{g}) \]
The equilibrium constant \( K \) for this reaction is 5.15 at the temperature of the flask.
**Objective:**
Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.
**Inputs:**
- Volume of the flask: 250 mL (0.250 L)
- Initial moles of Cl₂: 0.50 mol
- Initial moles of CHCl₃: 1.2 mol
- Initial moles of CCl₄: 0.80 mol
- Equilibrium constant \( K \): 5.15
**Instructions:**
Use the provided information to determine the equilibrium molarity of HCl in the flask.
**Interactive Elements:**
- A text box for input: \[ \boxed{M} \]
- Functional control buttons:
- Clear input: \[ \boxed{\times} \]
- Reset form: \[ \boxed{\curvearrowright} \]
- Help section: \[ \boxed{?} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F20b515c9-5e3a-448e-90a2-ac3b562e1523%2F7eef1000-590e-4028-8272-9e0b775f38c9%2F2pnytsn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemistry Equilibrium Calculation Example:**
**Problem Statement:**
Suppose a 250 mL flask is filled with 0.50 mol of Cl₂, 1.2 mol of CHCl₃, and 0.80 mol of CCl₄. The following reaction becomes possible:
\[ \text{Cl}_2(\text{g}) + \text{CHCl}_3(\text{g}) \rightleftharpoons \text{HCl}(\text{g}) + \text{CCl}_4(\text{g}) \]
The equilibrium constant \( K \) for this reaction is 5.15 at the temperature of the flask.
**Objective:**
Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.
**Inputs:**
- Volume of the flask: 250 mL (0.250 L)
- Initial moles of Cl₂: 0.50 mol
- Initial moles of CHCl₃: 1.2 mol
- Initial moles of CCl₄: 0.80 mol
- Equilibrium constant \( K \): 5.15
**Instructions:**
Use the provided information to determine the equilibrium molarity of HCl in the flask.
**Interactive Elements:**
- A text box for input: \[ \boxed{M} \]
- Functional control buttons:
- Clear input: \[ \boxed{\times} \]
- Reset form: \[ \boxed{\curvearrowright} \]
- Help section: \[ \boxed{?} \]
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