Phosphorus Pentachloride Decomposes to Phosphorus Trichloride at High Temperatures According $\mathrm { PCl } _ { 5 } ( \mathrm {~g} ) \rightleftharpoons \mathrm { PCl } _ { 3 } ( \mathrm {~g} ) + \mathrm { Cl } _ { 2 } ( \mathrm {~g} )$

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: $\mathrm { PCl } _ { 5 } ( \mathrm {~g} ) \rightleftharpoons \mathrm { PCl } _ { 3 } ( \mathrm {~g} ) + \mathrm { Cl } _ { 2 } ( \mathrm {~g} )$ At 250° 0.125 mol L^-1 PCl₅ is added to the flask.If K_c = 1.80 mol L^-1,what are the equilibrium concentrations of each gas?

A) [PCl₅] = 0.00765 mol L^-1,[PCl₃] = 0.117 mol L^-1,and [Cl₂] = 0.117 mol L^-1
B) [PCl₅] = 0.0625 mol L^-1,[PCl₃] = 0.335 mol L^-1,and [Cl₂] = 0.335 mol L^-1
C) [PCl₅] = 1.80 mol L^-1,[PCl₃] = 1.80 mol L^-1,and [Cl₂] = 1.80 mol L^-1
D) [PCl₅] = 3.96 mol L^-1,[PCl₃] = 3.83 mol L^-1,and [Cl₂] = 3.83 mol L^-1

Correct Answer:

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