Chem Help please

Question

At a certain temperature, a 27.5-L container holds four gases in equilibrium. Their masses are 3.5 g SO3 , 4.6 g SO2 , 19.5 g N2 , and 0.98 g N2O .

What is the value of the equilibrium constant at this temperature for the reaction of SO2 with N2O to form SO3 and N2? Make sure you balance the reaction using the lowest whole-number coefficients.

Kc=

Answer 1

Let us first convert mass of gas to moles and then to concentration;

3.5 g SO₃ x 1 mol / 80 g = 0.04375 mols SO₃ / 27.5 L = 0.00159 M

4.6 g SO₂ x 1 mol / 64 g = 0.07188 mols SO₂ = 0.00261 M

19.5 g N₂ x 1 mol / 28 g = 0.6964 mols N₂ = 0.0253

0.98 g N₂O x 1 mol / 44 g = 0.0218 mols N₂O = 0.000793 M

SO₂ + N₂O <==> SO₃ + N₂

Keq = [SO₃][N₂] / [SO²][N₂O]

Keq = (0.00159)(0.0253) / (0.00261)(0.000793)

Keq = 19.4

(be sure to check my math)