Question

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?

Answer 1

Answer:

a) kc= [SO3 ]/([SO2 ][O2 ])

b) kc= 2.27*10⁶ M⁻¹

v) the reaction is product-favored

Explanation:

for the reaction, the equilibrium constant is

SO2 (g) + O2 (g) <-----> SO3 (g)

he equilibrum constant is

kc= [SO3 ]/([SO2 ]*[O2 ])

replacing values

kc= [SO3 ]/([SO2 ]*[O2 ]) = 1.01*10⁻² M/(3.61*10⁻³M*6.11 x 10⁻⁴ M) = 2.27*10⁶ M⁻¹

since kc>>1 the reaction is product-favored