Question

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11. For the reaction, 2 SO2(g) + O2(g) - 2 SO3(g), at 450.0 K the equilibrium constant, Kc, has a value of 4.62. A system was charged to give these initial concentrations: (SO3) = 0.0254 M, [O2) = 0.00855 M. (SO2) = 0.500 M. In which direction will it go? a. to the right b. to the left c. to the right or the left depending on the pressure d. it will remain at the same concentrations e to the right or the left depending on the volume

Answer 1

2502 +02= 2503 K. – [SO3)2 [SO2]2[O2] at 450 K we have (SO3)2 (S0,1210,1 = 4.62 [SO3)= 4.62(SO2)2 [02] = 4.62 x (0.500)2 x 0.00855 = 9.875 x 10-3 [SO3] = 0.09937 From the value K. the equilibrium concentration of SO3 should be 0.09037 M.The initial concentration of SO3 is 0.0254 M which is less than the required equilibrium concentration of SO3, so following the Le Chatelier and Braun's principle the system will proceed towards right to attain the equilibrium concentration of SO3.