0.2000 mol each of SO2, O2 and SO3 is placed in a 2.000 L flask and allowed to come to equilibrium. The equilibrium [SO2] is found to be 0.0040 mol/L. What is the value of Keq for the reaction? 2 SO2(g) + O2(g) --> 2 SO3(g)
The equilibrium constant expression for this reaction is given by Keq = ([SO3]^2)/([SO2]^2[O2]).
We are given that the equilibrium [SO2] is 0.0040 mol/L. Since the initial moles of each reactant is 0.2000 mol and the flask volume is 2.000 L, the initial concentration of SO2 is 0.2000 mol/2.000 L = 0.1000 mol/L.
Substituting the given values into the equilibrium constant expression, we have:
Keq = ([SO3]^2)/([SO2]^2[O2]) = ([SO3]^2)/(0.1000^2[O2])
We don't have the equilibrium concentrations of [SO3] or [O2], so we cannot directly calculate Keq.