2.In the contact process, sulfuric acid is manufactured by first oxidizing SO2 to S03,that is then reacted with water. The reaction of SO2 with oxygen is:2 SO2 (g) 02 (g)2 SO3 (g)A 2.000 L flask was filled with 0.04000 mol SO2 and 0.02000 mol 02. At equilibrium at900K, the flask contained 0.0296 mol SO3.a)What is the value of Ke for this reaction at 900K?What is the equilibrium pressure of SO2 in the vessel?b)

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Asked Dec 1, 2019
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2.
In the contact process, sulfuric acid is manufactured by first oxidizing SO2 to S03,
that is then reacted with water. The reaction of SO2 with oxygen is:
2 SO2 (g) 02 (g)
2 SO3 (g)
A 2.000 L flask was filled with 0.04000 mol SO2 and 0.02000 mol 02. At equilibrium at
900K, the flask contained 0.0296 mol SO3.
a)
What is the value of Ke for this reaction at 900K?
What is the equilibrium pressure of SO2 in the vessel?
b)
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2. In the contact process, sulfuric acid is manufactured by first oxidizing SO2 to S03, that is then reacted with water. The reaction of SO2 with oxygen is: 2 SO2 (g) 02 (g) 2 SO3 (g) A 2.000 L flask was filled with 0.04000 mol SO2 and 0.02000 mol 02. At equilibrium at 900K, the flask contained 0.0296 mol SO3. a) What is the value of Ke for this reaction at 900K? What is the equilibrium pressure of SO2 in the vessel? b)

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Expert Answer

Step 1

Given,

Volume, V = 2 L

Temperature, T = 900 K

Initial moles of SO2 = 0.04 mol

Initial moles of O2 = 0.02 mol

Equilibrium moles of SO3 = 0.0296 mol

The given reaction is :

2 SO2 (g) + O2 (g) → 2 SO3 (g)

The ICE table for this reaction can be written as:

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2 SO2 2 SO3 O2 Initial moles (I) 0.02 0.04 0 Change (C) 2x +2x -X Equilibrium moles (E) 0.02-x 0.04-2x 2х 2x 0.0296 mol x= 0.0148 mol

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Step 2

At equilibrium, moles of SO2 and O2 are:

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Moles of SO2 = 0.04 mol - 2x = 0.04 mol - 2(0.0148 mol) = 0.0104 mol Moles of O2 0.02 mol - x= 0.02 mol - 0.0148 mol 0.0052 mol

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Step 3

Therefore, the equilibrium constant, KC...

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[SO312 Кс [SO2]2 [O2 (0.0296 mol/2 L)2 (0.0104 mol/2 L)2 (0.0052 mol/2 L) Кс (0.0148)2 Кс (0.0052)2 (0.0026) Kc 3115.61

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