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b. the system is at equilibrium, and dichlorine (Cl2) is added to the reaction (no change in volume). What is the resulting effect on the concentrations of PBr3, PCI3, and Br2 when the system regains equilibrium? [PBr3] [PC\3] [Br2|

b. the system is at equilibrium, and dichlorine (Cl2) is added to the reaction (no change in volume). What is the resulting effect on the concentrations of PBr3, PCI3, and Br2 when the system regains equilibrium? [PBr3] [PC\3] [Br2|

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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3b) please see attached

### Understanding Le Chatelier’s Principle Through Chemical Equilibrium Le Chatelier’s Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. Let’s explore this principle using the following chemical reaction which occurs with all substances in the gaseous state: #### Chemical Equation \[ \text{PBr}_3 + \text{Cl}_2 \leftrightarrow \text{PCl}_3 + \text{Br}_2 \] #### Equilibrium Constant The equilibrium constant (Kc) for this reaction is \(4.2 \times 10^2\) at 325°C. #### Enthalpy Change The standard enthalpy change (\(\Delta H^\circ\)) for this reaction is \(-47 \text{ kJ/mol}\). ### Analysis 1. **Equilibrium Constant (Kc):** - The value of \(4.2 \times 10^2\) indicates the ratio of product concentrations to reactant concentrations at equilibrium. - A high \(Kc\) value suggests that at 325°C, the equilibrium position is heavily shifted towards the products (\(\text{PCl}_3\) and \(\text{Br}_2\)). 2. **Reaction Conditions:** - All reactants and products are in the gaseous phase. - The reaction's equilibrium can be influenced by changes in temperature, pressure, and concentration of reactants or products. 3. **Enthalpy Change (\(\Delta H^\circ\)):** - The reaction is exothermic (\(\Delta H^\circ = -47 \text{ kJ/mol}\)), releasing heat to the surroundings. ### Application of Le Chatelier’s Principle 1. **Change in Concentration:** - Increasing the concentration of \(\text{PBr}_3\) or \(\text{Cl}_2\) would shift equilibrium towards the products (\(\text{PCl}_3\) and \(\text{Br}_2\)). - Increasing the concentration of \(\text{PCl}_3\) or \(\text{Br}_2\) would shift equilibrium towards the reactants (\(\text{PBr}_3\) and \(\text{Cl}_2\)). 2. **Change in Temperature:** - As the reaction is exothermic, increasing the temperature would shift
Transcribed Image Text:### Understanding Le Chatelier’s Principle Through Chemical Equilibrium Le Chatelier’s Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. Let’s explore this principle using the following chemical reaction which occurs with all substances in the gaseous state: #### Chemical Equation \[ \text{PBr}_3 + \text{Cl}_2 \leftrightarrow \text{PCl}_3 + \text{Br}_2 \] #### Equilibrium Constant The equilibrium constant (Kc) for this reaction is \(4.2 \times 10^2\) at 325°C. #### Enthalpy Change The standard enthalpy change (\(\Delta H^\circ\)) for this reaction is \(-47 \text{ kJ/mol}\). ### Analysis 1. **Equilibrium Constant (Kc):** - The value of \(4.2 \times 10^2\) indicates the ratio of product concentrations to reactant concentrations at equilibrium. - A high \(Kc\) value suggests that at 325°C, the equilibrium position is heavily shifted towards the products (\(\text{PCl}_3\) and \(\text{Br}_2\)). 2. **Reaction Conditions:** - All reactants and products are in the gaseous phase. - The reaction's equilibrium can be influenced by changes in temperature, pressure, and concentration of reactants or products. 3. **Enthalpy Change (\(\Delta H^\circ\)):** - The reaction is exothermic (\(\Delta H^\circ = -47 \text{ kJ/mol}\)), releasing heat to the surroundings. ### Application of Le Chatelier’s Principle 1. **Change in Concentration:** - Increasing the concentration of \(\text{PBr}_3\) or \(\text{Cl}_2\) would shift equilibrium towards the products (\(\text{PCl}_3\) and \(\text{Br}_2\)). - Increasing the concentration of \(\text{PCl}_3\) or \(\text{Br}_2\) would shift equilibrium towards the reactants (\(\text{PBr}_3\) and \(\text{Cl}_2\)). 2. **Change in Temperature:** - As the reaction is exothermic, increasing the temperature would shift
**Question b: Effect of Adding Dichlorine (Cl₂) to the Reaction at Equilibrium** The system is initially at equilibrium, and dichlorine (Cl₂) is added to the reaction while maintaining a constant volume. The objective is to analyze the resulting effect on the concentrations of PBr₃, PCl₃, and Br₂ once the system re-establishes equilibrium. The specific aspects to consider are: - **[PBr₃]**: What is the concentration of phosphorus tribromide (PBr₃) after equilibrium is re-established? - **[PCl₃]**: What is the concentration of phosphorus trichloride (PCl₃) after equilibrium is re-established? - **[Br₂]**: What is the concentration of bromine (Br₂) after equilibrium is re-established? When Cl₂ is added to the reaction system at equilibrium, it will temporarily disturb the equilibrium, and the system will adjust to minimize this disturbance, according to Le Chatelier's Principle. The analysis will involve understanding the reaction dynamics and predicting the direction of the shift in equilibrium to determine the new concentrations of PBr₃, PCl₃, and Br₂. In summary, adding Cl₂ to the equilibrium system typically shifts the reaction direction in such a way that counters the increased concentration of Cl₂, thereby affecting the concentrations of the other reactants and products accordingly. --- The remainder of the page appears to be reserved for calculations or space to write the determined concentrations following the analysis. If any graphs or diagrams had been provided, they would serve to illustrate the shift in equilibrium concentrations and the dynamic response of the system to the addition of Cl₂. However, no such visual aids are present in this case.
Transcribed Image Text:**Question b: Effect of Adding Dichlorine (Cl₂) to the Reaction at Equilibrium** The system is initially at equilibrium, and dichlorine (Cl₂) is added to the reaction while maintaining a constant volume. The objective is to analyze the resulting effect on the concentrations of PBr₃, PCl₃, and Br₂ once the system re-establishes equilibrium. The specific aspects to consider are: - **[PBr₃]**: What is the concentration of phosphorus tribromide (PBr₃) after equilibrium is re-established? - **[PCl₃]**: What is the concentration of phosphorus trichloride (PCl₃) after equilibrium is re-established? - **[Br₂]**: What is the concentration of bromine (Br₂) after equilibrium is re-established? When Cl₂ is added to the reaction system at equilibrium, it will temporarily disturb the equilibrium, and the system will adjust to minimize this disturbance, according to Le Chatelier's Principle. The analysis will involve understanding the reaction dynamics and predicting the direction of the shift in equilibrium to determine the new concentrations of PBr₃, PCl₃, and Br₂. In summary, adding Cl₂ to the equilibrium system typically shifts the reaction direction in such a way that counters the increased concentration of Cl₂, thereby affecting the concentrations of the other reactants and products accordingly. --- The remainder of the page appears to be reserved for calculations or space to write the determined concentrations following the analysis. If any graphs or diagrams had been provided, they would serve to illustrate the shift in equilibrium concentrations and the dynamic response of the system to the addition of Cl₂. However, no such visual aids are present in this case.
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