At a certain temperature, 0.920 mol of SO3 is placed in a 2.50-L container.
2 SO3 (g) ⇌ 2 SO2 (g) + O2 (g)
At equilibrium, 0.140 mol of O2 is present. Calculate Kc.
At a certain temperature, 0.920 mol of SO3 is placed in a 2.50-L container.
2 SO3 (g) ⇌ 2 SO2 (g) + O2 (g)
The equilibrium constant will relate product and reactants distribution. It is similar to a ratio
The equilibrium is given by
rReactants -> pProducts
Keq = [products]^p / [reactants]^r
For a specific case:
aA + bB = cC + dD
Keq = [C]^c * [D]^d / ([A]^a * [B]^b)
now...
Keq = [SO2]^2 [ O2 ] /[SO3]^2
initial conditions
[SO2] = 0
[O2] = 0
[SO3] = mol/V = 0.92/2.5 = 0.368 M
in equilibrium
[SO2] = 0 + 2x
[O2] = 0 + x
[SO3] = 0.368 -2x
and we know
At equilibrium, 0.140 mol of O2 is present. Calculate Kc.
[O2] = 0 + x = mol/V
x = 0.14/2.5 = 0.056
substitute
[SO2] = 0 + 2*0.056 = 0.112 M
[O2] = 0 + 0.056 = 0.056 M
[SO3] = 0.368 -2*0.056 = 0.256 M
Keq = [SO2]^2 [ O2 ] /[SO3]^2
Keq = (0.112 ^2)* (0.056 ) /(0.256 ^2)
Keq = 0.01071875
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