Given the concentrations, calculate the equilibrium constant for this reaction:

Question

Given the concentrations, calculate the equilibrium constant for this reaction: PCl3(g) + Cl2(g) PCl5(g) At equilibrium, the molar concentrations for reactants and products are found to be [PCI3] = 0.20 M. [Cl2] = 0.25 M and [PCl5] = 1.20 M What a the equilibrium constant (Kc) for this reaction? The concentration of PCl3(g) is increased to 1 2 M. disrupting equilibrium. Calculate the new ratio of products to reactants with this higher concentration of phosphorus trichloride. Assume that the reaction has not yet regained equilibrium.

Explanation / Answer

PCl3 + Cl2 --> PCl5

[PCl3 ]= 0.2

[Cl2 ]= 0.25

[PCl5] = 1.20

Find Kc

Kc = [PCl5]/[PCl3 ][Cl2 ]

Kc = (1.20) / (0.25*0.20 ) = 24

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