c. the system is at equilibrium and helium gas (He) is added to the reaction. What is the effect on the concentrations of PB13, PCI3, Cl2, and Brz when the system regains equilibrium? [PB33| (Cl2] [PCI3 ] [Br2]
c. the system is at equilibrium and helium gas (He) is added to the reaction. What is the effect on the concentrations of PB13, PCI3, Cl2, and Brz when the system regains equilibrium? [PB33| (Cl2] [PCI3 ] [Br2]
Chemistry
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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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3c) please see attached
![**Question:**
The system is at equilibrium and helium gas (He) is added to the reaction. What is the effect on the concentrations of PBr₃, PCl₃, Cl₂, and Br₂ when the system regains equilibrium?
\[ \text{[PBr}_3\text{]} \quad \text{[Cl}_2\text{]} \quad \text{[PCl}_3\text{]} \quad \text{[Br}_2\text{]} \]
**Explanation:**
In an equilibrium system, adding an inert gas such as helium generally does not affect the concentrations of the reactants and products because helium does not react with the chemical species in the system. Therefore, when helium is added to the reaction at equilibrium:
- \[ \text{[PBr}_3\text{]} \]: No change
- \[ \text{[Cl}_2\text{]} \]: No change
- \[ \text{[PCl}_3\text{]} \]: No change
- \[ \text{[Br}_2\text{]} \]: No change
These concentrations will remain the same when the system regains equilibrium after the addition of helium.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F48deb947-3d41-43de-ac43-bef03e01cc59%2F2e7037cc-6a52-40f3-a884-21b63d21b444%2Fcp9636g.png&w=3840&q=75)
Transcribed Image Text:**Question:**
The system is at equilibrium and helium gas (He) is added to the reaction. What is the effect on the concentrations of PBr₃, PCl₃, Cl₂, and Br₂ when the system regains equilibrium?
\[ \text{[PBr}_3\text{]} \quad \text{[Cl}_2\text{]} \quad \text{[PCl}_3\text{]} \quad \text{[Br}_2\text{]} \]
**Explanation:**
In an equilibrium system, adding an inert gas such as helium generally does not affect the concentrations of the reactants and products because helium does not react with the chemical species in the system. Therefore, when helium is added to the reaction at equilibrium:
- \[ \text{[PBr}_3\text{]} \]: No change
- \[ \text{[Cl}_2\text{]} \]: No change
- \[ \text{[PCl}_3\text{]} \]: No change
- \[ \text{[Br}_2\text{]} \]: No change
These concentrations will remain the same when the system regains equilibrium after the addition of helium.
![**Le Chatelier's Principle: Equilibrium Constant and Thermodynamics of the Reaction**
The following chemical reaction is discussed under the principles of Le Chatelier:
\[ \text{PBr}_3 + \text{Cl}_2 \rightleftharpoons \text{PCl}_3 + \text{Br}_2 \]
### Equilibrium Constant (Kc)
The equilibrium constant (Kc) of this reaction at 325°C is given as:
\[ K_c = 4.2 \times 10^2 \]
### Thermodynamic Information
The enthalpy change (ΔHº) for the reaction is:
\[ \Delta H^\circ = -47 \, \text{kJ/mol} \]
### Key Points:
- All substances involved in this reaction are in the gaseous state.
- The given equilibrium constant indicates the ratio of the concentrations of the products to the reactants at equilibrium.
- The negative enthalpy change indicates that the reaction is exothermic, releasing energy in the form of heat.
This reaction and its thermodynamic properties can be used to understand how changes in temperature and concentration will affect the position of the equilibrium, as per Le Chatelier's Principle.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F48deb947-3d41-43de-ac43-bef03e01cc59%2F2e7037cc-6a52-40f3-a884-21b63d21b444%2Fg8aawf.png&w=3840&q=75)
Transcribed Image Text:**Le Chatelier's Principle: Equilibrium Constant and Thermodynamics of the Reaction**
The following chemical reaction is discussed under the principles of Le Chatelier:
\[ \text{PBr}_3 + \text{Cl}_2 \rightleftharpoons \text{PCl}_3 + \text{Br}_2 \]
### Equilibrium Constant (Kc)
The equilibrium constant (Kc) of this reaction at 325°C is given as:
\[ K_c = 4.2 \times 10^2 \]
### Thermodynamic Information
The enthalpy change (ΔHº) for the reaction is:
\[ \Delta H^\circ = -47 \, \text{kJ/mol} \]
### Key Points:
- All substances involved in this reaction are in the gaseous state.
- The given equilibrium constant indicates the ratio of the concentrations of the products to the reactants at equilibrium.
- The negative enthalpy change indicates that the reaction is exothermic, releasing energy in the form of heat.
This reaction and its thermodynamic properties can be used to understand how changes in temperature and concentration will affect the position of the equilibrium, as per Le Chatelier's Principle.
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