6. You place 3.00 mol of pure SOs in an 8.00 L flask at 1150 K. At equilibrium,
ID: 1036422 • Letter: 6
Question
6. You place 3.00 mol of pure SOs in an 8.00 L flask at 1150 K. At equilibrium, 0.58 mol of O2 has been formed. Calculate Kc for the reaction at 1150 K. (Hint: Must calculate the molarities) (6 pts) 2SOfg) 2so3(g) + 02(g) 7. The reaction: N2(g) burned at a high temperature, as in a gasoline engine. At 1500 K, K-1.0 x 105.Suppose a sample of air has [N2] = 0.80 M and [02] = 0.20 M before any reaction occurs Calculate the equilibrium concentrations of N2, O2 and NO after the mixture has been heated to 1500 K (8 pts) O2(g) 2 NO(g) contributes to air pollution whenever a fuel is +Explanation / Answer
Initial concentration SO3 = 3.00 mol / 8.00L = 0.375 M
Concentration O2 at equlibrium = 0.58 mol / 8.00 = 0.0725 M
2 SO3 <-----> 2SO2 + O2
initial concentration
0.375 0 0
change
-2x. . . . . . . . .. +2x. . . .+x
at equilibrium
0.375-2x . . . .. . 2x. . . . .. x
x = 0.0725
2x = 0.145
concentration SO3 = 0.375 - 0.145 = 0.230 M
K = (0.145)^2 ( 0.0725) / (0.230)^2 = 0.0288.
Post seprately (question 2) for detailed solution.
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