At a certain temperature, 0.980 mol SO3 is placed in a 4.00 L container.
2SO3(g)−⇀↽−2SO2(g)+O2(g)
At equilibrium, 0.180 mol O2 is present. Calculate Kc.
Answer:
Step 1: Explanation
Kc is defined as the amounts of products and reactants present at equilibrium in a reversible chemical reaction at a given temperature
Step 2: Write the balanced the chemical equation
2SO3 (g) <--------------> 2SO2 (g)+O2(g)
Step 3: Calculate the Concentrations by dividing the given moles by volume of container.
Given,
Initial SO3 = moles / volume = (0.980 moles / 4 litre ) = 0.245 M
as well the concentration of O2 at equilibrium = ( 0.180 moles / 4 L ) = 0.045 M
Step 3: Write the ICE table
2SO3 (g) <--------------> 2SO2 (g) + O2(g)
Initial amount 0.245 0 0
Change amount -2x +2x +x
Equilibrium amount 0.245-2x 2x x
Since the value of O2 at equlibrium is given [O2] = 0.045 M = [x]
hence value of x = 0.045 M
Hence all value at equilibrium is
[SO3] = 0.245 -2x = 0.245 -(2 × 0.045 ) =0.155
[SO2] = 2x = 2 × 0.045 = 0.09
[O2] = x = 0.045
Step 4: Calculate the Kc
2SO3 (g) <--------------> 2SO2 (g) + O2(g)
The Kc expression will be
Kc = [SO2]2 × [O2] / [SO3]2
on substituting the value
Kc= ( 0.09)2×(0.045) / (0.155)2 = 0.0151717 ≈ 1.52 ×10-2
Hence, the value of Kc = 0.0151717 ≈ 1.52 ×10-2
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