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:**- \([\text{PBr}_3] = [\text{Cl}_2] = 0.0273 \, \text{M}\)- \([\text{PCl}_3] = [\text{Br}_2] = 0.560 \, \text{M}\)### QuestionWhat 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 PrincipleGiven 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

The nature of the reaction is exothermic it means that if the reaction proceeds in a forward…

(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]