An equilibrium mixture at 852 K is found to contain 3.61 x 10^ - 3 mol/L SO3. Calculate the equililbrium , constant , keq for the reaction where SO2 an O2 are reactants and SO3 is the produce.

2SO2 + O2 ==> 2SO3

equilibrium:
SO3 = 3.61 x 10^-3 M

SO3 must be the same (the coefficients are the same).
O2 must be 1/2 the value (2 moles SO3 = 1 mole O2).
Substitute into Keq and solve for Kc.

i got 2.83 is that correct??

I don't have 2.83

Kc = (SO3)^2/(SO2)^2(O2)
Substitute into this.

isnt the numerator supposed to be (2)SO3^2?

and same with SO2

To calculate the equilibrium constant, Kₑq, for the given reaction, you will need the balanced chemical equation and the concentration of the reactants and products at equilibrium.

The balanced chemical equation for the reaction is:

2 SO2 + O2 ⇌ 2 SO3

First, we need to determine the concentrations of the reactants and products at equilibrium. From the given information, we know that the concentration of SO3 at equilibrium is 3.61 × 10^(-3) mol/L.

Since the stoichiometric coefficients for SO3 in the balanced equation are equal on both sides, the concentration of SO2 and O2 at equilibrium will also be 0. We assume the initial concentrations of SO2 and O2 to be zero.

Now, we can substitute the equilibrium concentrations into the equilibrium expression to calculate Kₑq. The equilibrium expression for the given reaction is:

Kₑq = [SO3]² / ([SO2]² × [O2])

Substituting the values:

Kₑq = (3.61 × 10^(-3))² / ((0)² × (0))

Since both [SO2] and [O2] are zero at equilibrium, the equilibrium constant for this reaction cannot be determined because it will involve division by zero.

Therefore, in this case, the equilibrium constant, Kₑq, is undefined.