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The equilibrium concentrations of the reactants and products were measured for the following chemical reaction. PCl3(g)...

The equilibrium concentrations of the reactants and products were measured for the following chemical reaction. PCl3(g) + Cl2(g) equilibrium reaction arrow PCl5(g) equilibrium concentrations: [PCl3] = 0.203 M [Cl2] = 0.203 M [PCl5] = 0.939 M At a certain temperature, the equilibrium constant, Kc, for this reaction, is 94.1. If an additional 0.250 M PCl3 is added to the system, determine the new equilibrium concentrations of PCl3, Cl2, and PCl5.

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Expert Solution

                       PCl3(g) + Cl2(g) --------------->PCl5(g)

                      0.453    0.203                         0.939

                      -x               -x                               +x

                   0.453-x        0.203-x                     0.939+x

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

                            94.1 = (0.939+x)/(0.453-x)*(0.203-x)

                          94.1*(0.453-x)*(0.203-x)    = (0.939+x)

                                   x    = 0.163

                       [PCl3]   = 0.453-x   = 0.453-0.163   = 0.29M

                        [Cl2]     = 0.203-x   = 0.203-0.163   = 0.04M

                     [PCl5]      = 0.939+x   = 0.939+0.163   = 1.102 M

                   

queen_honey_blossom answered 2 years ago
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