If this equation has reached equilibrium, what is the effect of lowering the temp: PCl3(g) + Cl2(g) ↔ PCl5(g)

Question

Will more PCl5 form? Will the reverse and forward reaction rates both decrease? Will the reverse reaction be favored? Will more More PCl3, Cl2, and PCl5 form? Or, will the equilibrium just be unaffected?

Answer 1

If the reaction is endothermic (has a positive heat if reaction) then increasing the temperature would favor the production of phosphorus pentachloride,. In this case the forward rate of reaction will increase until a new equilibrium is reached where the forward and reverse rate of reactions will be the same.

Answer 2

PCl3(g) + Cl2(g) ? PCl5(g) + skill in accordance to the Le Chatelier's theory, while a equipment at equilibrium is subjected to a "tension", it reacts through moving in in spite of path mandatory to alleviate the outcomes of the strain. in accordance to the above assertion, if between the reactants or products is faraway from the equipment, the equipment will attempt to offer extra of it. If between the reactants or products is extra to the equipment, the equipment will attempt to apply it up. because of the fact the observe "exothermic reaction" is secure interior the question, it likely refers back to the forward reaction, and the "skill" term could desire to look on the area of the products. It acts in simple terms as a reactant or a product, while the equipment is decrease than "tension". The temperature is diminished, warmth (skill) is faraway from the equipment at equilibrium. The equipment will attempt to offer extra warmth (skill) to interchange it through dashing up the forward reaction. This in turn will decrease the quantity of phosphorus trichloride and chlorine, and advance the quantity of phosphorus pentachloride. A. The opposite reaction is favorite. because of the fact that through removing warmth, the equilibrium will shift to the terrific (forward), the above assertion is fake. B. The opposite and forward reaction expenditures the two decrease. because of the fact that through removing warmth, the equilibrium will shift to the terrific (forward), no longer the two strategies, the above assertion is fake. C. extra PCl3, Cl2, and PCl5 varieties. because of the fact that through removing warmth, the equilibrium will shift to the terrific (forward), no longer the two strategies, basically the quantity of the product (phosphorus pentachloride) will advance, mutually as quantities of phosphorus trichloride and chlorine (reactants) will decrease, and the above assertion is fake. D. extra PCl5 varieties. because of the fact that through removing warmth, the equilibrium will shift to the terrific (forward), the quantity of the product (phosphorus pentachloride) will advance, and the above assertion is authentic. E. Equilibrium is unaffected. because of the fact that through removing warmth, the equilibrium will shift to the terrific (forward), and the quantity of the product (phosphorus pentachloride) will advance, mutually as quantities of phosphorus trichloride and chlorine (reactants) will decrease, so the above assertion is fake. answer: D. extra PCl5 varieties.

Answer 3

If this reaction is exothermic (you will need to check) then lowering the temperature will make more PCl5.