Question

Consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) A reaction mixture is made containing an initial [SO2Cl2] of 2.2×10−2M . At equilibrium, [Cl2]= 1.3×10−2M .

Answer 1

The value of the equilibrium constant, Ke, for the given reaction is 3.37.

Step-by-step explanation:

The equilibrium constant, Ke, can be calculated using the concentrations at equilibrium. The equation for the reaction is 2SO2(g) + O2(g) → 2SO3(g). Given that [SO2] = 0.90 M, [O2] = 0.35 M, and [SO3] = 1.1 M, we can plug these values into the equilibrium expression Ke = ([SO3]^2) / ([SO2]^2 * [O2]). Substituting the given values gives us Ke = (1.1^2) / (0.90^2 * 0.35) = 3.37.

Answer 2

I think you want to ask about Keq. At equilibrium, we can know [SO2Cl2] is 2.2*10-2 M -1.3*10-2M=9*10^-3 M. And [SO2]=[Cl2]. So the Keq=1.88*10^-2.