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.

Question

At a certain temperature, a  container holds four gases in equilibrium. Their masses are  g ,  g ,  g , and  g .

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.

Answer 1

SO₂ + N₂O ==> SO₃ + N_{2 ...} balanced equation

moles SO₃ = 3.5 g x 1 mol/80 g = 0.04375 moles

moles N₂ = 11.3 g x 1 mol/28 g = 0.4036 moles

moles SO₂ = 4.6 g x 1 mol/64 g = 0.0719 moles

moles N₂O = 0.98 g x 1 mol/44 g = 0.0223 moles

At equilibrium, the concentration are as follows:

[SO₃] = 0.04375 mol/22.5 L = 0.0019 M

[N₂] = 0.4036 mol/22.5 L = 0.018 M

[SO₂] = 0.0719 mol/22.5 L = 0.0032 M

[N₂O] = 0.0223 mol/22.5 L = 0.00099 M

K = [SO₃][N₂] / [SO₂][N₂O] = (0.0019)(0.018) / (0.0032)(0.00099)

K = 10.8 = 11 (2 significant figures)