Solution:
For the given reaction, ICE table can be written as,
2SO3 (g) = 2SO2 (g) + O2 (g)
0.840 mol --------0 mol ---------0 mol (initial)
- 2X ---------------- +2X ------------+X (change)
(0.840 - 2X)--------- 2X ------------- X (equilibrium)
Kc of the given reaction can be calculated from ICE table as,
Given, X = 0.130 mol
Then,
Number of moles of SO3 = 0.840 - 2X = 0.840 -2 x.0.130
= 0.840 - 0.260 = 0.580 mol
[SO3] = 0.580 mol / 5 L = 0.116 M
Number of moles of SO2 = 2 X = 2 x 0.130 = 0.260 mol
[SO2] = 0.260 mol /5L = 0.052 M
[O2] = 0.130 mol / 5 L = 0.026 M
Thus,
Kc = [SO2]^2 [O2] / [SO3]^2
Kc = (0.052)^2 x ( 0.026) / (0.116)^2
Kc = 0.00523
OR
Kc = 5.23 x 10^-3
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