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?

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Quizplus · Accepted Answer

The equilibrium constant expression is:$$K_c = \frac{[\mathrm{PCl}_3][\mathrm{Cl}_2]}{[\mathrm{PCl}_5]}$$Substituting the given values into the equilibrium constant expression, we get:$$1.80 = \frac{[\mathrm{PCl}_3][\mathrm{Cl}_2]}{0.125}$$Solving for [PCl₃] and [Cl₂], we get:$$[\mathrm{PCl}_3] = [\mathrm{Cl}_2] = 0.117 ext{ mol L}^{-1}$$Therefore, the equilibrium concentrations are:$$[\mathrm{PCl}_5] = 0.00765 ext{ mol L}^{-1}$$$$[\mathrm{PCl}_3] = 0.117 ext{ mol L}^{-1}$$$$[\mathrm{Cl}_2] = 0.117 ext{ mol L}^{-1}$$

Phosphorus Pentachloride Decomposes to Phosphorus Trichloride at High Temperatures According PCl5( g)⇌PCl3( g)+Cl2( g)\mathrm { PCl } _ { 5 } ( \mathrm {~g} ) \rightleftharpoons \mathrm { PCl } _ { 3 } ( \mathrm {~g} ) + \mathrm { Cl } _ { 2 } ( \mathrm {~g} )PCl5​( g)⇌PCl3​( g)+Cl2​( g)

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