Question
Law of Chemical Equilibrium and LeChatelier's Principle Pre-Lab Questions 1. For the reaction PCI_3(g) PCI_3(g) at 25degreeC the equilibrium concentrations were as follows: [PCI_3] = 7.2 M, [PCI_5] = 0.050 M, and [CI_2] = 7.2 M. Calculate the equilibrium constant for the reaction. 2. The dissociation of H1 to H_2 and I_2 is endothermic. If the reaction is at equilibrium predict in which direction the equilibrium shifts, right toward H_2 and I_2 or left toward H1, when the following stresses are applied. 2 H1(g) H_2(g) + I_2(g)
Explanation / Answer
Solution :-
PCl3 + Cl2 ------ > PCl5
Equilibrium concentrations
[PCl3] = 7.2 M
[Cl2]= 7.2 M
[PCl5]= 0.05 M
Equilibrium constant equation is as follows
Kc= [PCl5] / [PCl3][Cl2]
Kc=[0.05] / [7.2][7.2]
Kc= 9.65*10^-4
So the equilibrium constant for the reaction 9.65*10^-4