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?

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

d.) circle motion requires a force to give it a centripetal acceleration.

in scientific notation, the value of the  speed of light in a vacuum

  will be written as 2.995 * 10^8. when this value is represented in the form of

  a * 10^b, then, a = 2.995 and b = 8.

the value of the speed of light in a vacuum given above can also be rounded up to approximately 300000000. in this case, the scientific notation will be written as 3 *10^8.