Final answer:
To calculate the equilibrium constant Ke for the reaction 2SO2(g) + O2(g) ⇒ 2SO3(g), we use the change in concentration of the reactants and products at equilibrium. The equilibrium constant expression Ke is computed as [SO3]^2 / ([SO2]^2 x [O2]), and we substitute the equilibrium concentrations to get the value of Ke.
Step-by-step explanation:
To determine the equilibrium constant for the reaction 2SO2(g) + O2(g) ⇒ 2SO3(g), we can use the given equilibrium concentrations to calculate the equilibrium constant expression, Ke. According to the reaction stoichiometry, the change in concentration for SO2 will be twice that for O2, since it appears with a coefficient of 2 in the balanced equation. The decrease in SO2 concentration also equals the increase in SO3 concentration for the same reason.
Given the initial concentration of 1.00 M for SO2 and O2 and the equilibrium concentration of SO2 being 0.075 M, the change in SO2 concentration is 1.00 M - 0.075 M = 0.925 M. Since the reaction produces 2 moles of SO3 for every 2 moles of SO2 consumed, the equilibrium concentration of SO3 will be 0.925 M. As for O2, half the amount of SO2 is used, hence the decrease in O2 concentration will be 0.925 M / 2 = 0.4625 M. This gives us an equilibrium concentration for O2 of 1.00 M - 0.4625 M = 0.5375 M.
The equilibrium constant expression for the reaction is Ke = [SO3]2 / ([SO2]2 x [O2]). Plugging in the values gives us Ke = (0.925 M)2 / ((0.075 M)2 x (0.5375 M)), from which we can calculate the equilibrium constant Ke for the reaction of SO2 and O2.