The following (unbalanced) reaction is one of the steps to producing acid rain [as h2so4(aq)] from sulfur-containing coal. in a study of this reaction, a flask contains an equilibrium concentration of the three substances so2(g), o2(g) and so3(g) held at a constant temperature.

so2 (g) + o2 (g) < > so3 (g)

the concentrations at equilibrium are found to be: [so2] = 3.61 x 10-3m [o2] = 6.11 x 10-4 m [so3] = 1.01 x 10-2 m

(a) write the equilibrium constant expression, kc for this specific reaction.
(b) calculate the value of kc for this temperature.
(c) would you classify this as a product-favored reaction?