Question

Consider the reaction: SO2Cl2(g) SO2(g) + Cl2(g) Kc = 2.99 x 10-7 (at 227oC) A reaction mixture initially contains 0.175 M SO2Cl2 and no SO2 and Cl2. What is the equilibrium concentration of Cl2 at this temperature (227oC)? Use the assumption that x is small compared to the initial concentration of reactant.

Answer 1

SO2 I MM Answer) The given equation is an follows: So, ₂ (g) ² SO2(g) + ₂ (9) w we have to construct ICE table which is as follows - Sozda i - ₂ I 0.175M T OM I OM at -xm -UM tum +4 и El (0:175-V) in na Now the equilibrium constant ke can be expressed in terms of concentration as ke= [S0₂ ] [ 2 . [so, ela er, 2.99 x 107 = _Hox 00:175-X) Neglecting the value of a with respect of 0.17s we get, 2.99x107 - 0.175 or, m? = 2.99 x 107 x 0.175 ..^= (2•287 x109)M is [ex] = AM = (2+287x104) . The equilibrium concentration of el is (2.2878107) M. (Ansorer)