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(LeChatlier's principle) The following reaction has Kc = 4.2 x 10ʻ at 325°C, all gases. PBr3 + Ch - PCI3 + Brz AH° = -47 kJ/mol For this reaction at equilibrium, [PBr3] = [Cl2] = 0.0273 M, and [PCl;] = [Brz] = 0.560 M. What do you expect to happen to the equilibrium concentrations of each species (increase, decrease, stay the same) if the temperature of the reaction is raised to 450°C ? [PBr3| [Clz] [PCI3] [Br2]

(LeChatlier's principle) The following reaction has Kc = 4.2 x 10ʻ at 325°C, all gases. PBr3 + Ch - PCI3 + Brz AH° = -47 kJ/mol For this reaction at equilibrium, [PBr3] = [Cl2] = 0.0273 M, and [PCl;] = [Brz] = 0.560 M. What do you expect to happen to the equilibrium concentrations of each species (increase, decrease, stay the same) if the temperature of the reaction is raised to 450°C ? [PBr3| [Clz] [PCI3] [Br2]

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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3a) please see attached

## Le Chatelier's Principle in Chemical Equilibria **The following reaction has a \(K_c\) = \(4.2 \times 10^4\) at \(325^\circ \text{C}\), all gases:** \[ \text{PBr}_3 + \text{Cl}_2 \rightleftharpoons \text{PCl}_3 + \text{Br}_2 \] \[ \Delta H^\circ = -47 \, \text{kJ/mol} \] **Given Conditions at Equilibrium:** - \([\text{PBr}_3] = [\text{Cl}_2] = 0.0273 \, \text{M}\) - \([\text{PCl}_3] = [\text{Br}_2] = 0.560 \, \text{M}\) ### Question What do you expect to happen to the equilibrium concentrations of each species (increase, decrease, stay the same) if the temperature of the reaction is raised to \(450^\circ \text{C}\)? ### Analysis Using Le Chatelier's Principle Given that the reaction is exothermic (\(\Delta H^\circ = -47 \, \text{kJ/mol}\)), increasing the temperature will shift the equilibrium to the left to counteract the added heat. Consequently, the concentrations of the reactants and products will adjust as follows: - **\([\text{PBr}_3]\)**: **Increase** (since the equilibrium shifts towards the reactants) - **\([\text{Cl}_2]\)**: **Increase** (since the equilibrium shifts towards the reactants) - **\([\text{PCl}_3]\)**: **Decrease** (since the equilibrium shifts away from the products) - **\([\text{Br}_2]\)**: **Decrease** (since the equilibrium shifts away from the products) ### Summary of Expected Changes - **\[ \text{PBr}_3 \]**: Increase - **\[ \text{Cl}_2 \]**: Increase - **\[ \text{PCl}_3 \]**: Decrease - **\[ \text{Br}_2 \]**: Decrease
Transcribed Image Text:## Le Chatelier's Principle in Chemical Equilibria **The following reaction has a \(K_c\) = \(4.2 \times 10^4\) at \(325^\circ \text{C}\), all gases:** \[ \text{PBr}_3 + \text{Cl}_2 \rightleftharpoons \text{PCl}_3 + \text{Br}_2 \] \[ \Delta H^\circ = -47 \, \text{kJ/mol} \] **Given Conditions at Equilibrium:** - \([\text{PBr}_3] = [\text{Cl}_2] = 0.0273 \, \text{M}\) - \([\text{PCl}_3] = [\text{Br}_2] = 0.560 \, \text{M}\) ### Question What do you expect to happen to the equilibrium concentrations of each species (increase, decrease, stay the same) if the temperature of the reaction is raised to \(450^\circ \text{C}\)? ### Analysis Using Le Chatelier's Principle Given that the reaction is exothermic (\(\Delta H^\circ = -47 \, \text{kJ/mol}\)), increasing the temperature will shift the equilibrium to the left to counteract the added heat. Consequently, the concentrations of the reactants and products will adjust as follows: - **\([\text{PBr}_3]\)**: **Increase** (since the equilibrium shifts towards the reactants) - **\([\text{Cl}_2]\)**: **Increase** (since the equilibrium shifts towards the reactants) - **\([\text{PCl}_3]\)**: **Decrease** (since the equilibrium shifts away from the products) - **\([\text{Br}_2]\)**: **Decrease** (since the equilibrium shifts away from the products) ### Summary of Expected Changes - **\[ \text{PBr}_3 \]**: Increase - **\[ \text{Cl}_2 \]**: Increase - **\[ \text{PCl}_3 \]**: Decrease - **\[ \text{Br}_2 \]**: Decrease
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