At a certain temperature, 0.800 mol of SO3 is placed in a 2.00-L container.
2so3<->2so2 +o2
At equilibrium, 0.140 mol of O2 is present. Calculate Kc.
0.800 mol/2.00L = 0.400M
........2SO3 <==> 2SO2 + O2
I.....0.400M........0.....0
C.......-2x........2x.....x
E.....0400-2x......2x.....x
x = O2 = 0.140mol/2.00L = 0.07M
Then 2x = 0.140M = (SO2)
and 0.400-0.140 = 0.26M = (SO3)
Substitute these into the Kc expression and solve for Kc.
To calculate the equilibrium constant, Kc, for the given reaction, you need to determine the concentrations of the reactants and products at equilibrium.
First, you need to determine the number of moles of SO2 and O2 present. According to the balanced equation, for every 2 moles of SO3, we get 2 moles of SO2 and 1 mole of O2.
Given:
Initial moles of SO3 = 0.800 mol
Moles of O2 at equilibrium = 0.140 mol
Using stoichiometry, we can determine the number of moles of SO2 produced:
0.800 mol SO3 * (2 mol SO2 / 2 mol SO3) = 0.800 mol SO2
Now we have the moles of SO2, which is also present at equilibrium.
Now we can calculate the concentrations (in mol/L) of SO2, O2, and SO3:
[SO2] = 0.800 mol SO2 / 2.00 L = 0.400 M
[O2] = 0.140 mol O2 / 2.00 L = 0.070 M
[SO3] = 0.800 mol SO3 / 2.00 L = 0.400 M
Now we can calculate Kc using the formula for equilibrium constant:
Kc = ([SO2]^2 * [O2]) / [SO3]
= (0.400 M)^2 * 0.070 M / (0.400 M)
= 0.028 * 0.070 M
= 0.00196 M^2
So, the value of Kc is 0.00196 M^2.