Given the following decomposition reaction: PCl₅ (g) $\rightarrow$PCl₃ (g) + Cl₂ (g), when 0.84 moles of PCl₅ is placed in a 1.0 it was found that when the reaction reaches equilibrium, 0.72 moles of PCl₅ still remains. What is the value of the equilibrium constant for this reaction?

Question

Quizplus · Accepted Answer

The equilibrium constant (Kc) for a reaction is calculated using the concentrations of the reactants and products at equilibrium. In this case, the equilibrium concentrations are:[PCl5] = 0.72 M[PCl3] = (0.84 - 0.72) = 0.12 M[Cl2] = 0.12 MKc = [PCl3][Cl2]/[PCl5] = (0.12)(0.12)/(0.72) = 0.020

Given the Following Decomposition Reaction: PCl5 (G) →\rightarrow→ PCl3 (G) + Cl2 (G), When 0

Given the Following Decomposition Reaction: PCl₅ (G) $\rightarrow$ PCl₃ (G) + Cl₂ (G), When 0