Question

t a certain temperature, a 16.5-L contains holds four gases in equilibrium. Their masses are: 3.5...

t a certain temperature, a 16.5-L contains holds four gases in equilibrium. Their masses are: 3.5 g SO3, 4.6 g SO2, 15.3 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 (balanced with lowest whole-number coefficients)?

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Answer #1

Answer'

Chemical reaction

SO2 + N2O <-----> SO3 + N2

equilibrium constant ((Keq) = [SO3][N2] / [SO2][N2O] -----1)

molar concentrations can be calculated as

Molarity = No. of moles / volume in liters

No. of moles = given mass / molar mass

Volume = 16.5L

Molarity of SO2

No. of moles of SO2 = mass / molar mass = 4.6 / 64 = 0.072 moles

Molarity of SO2 = 0.072 / 16.5 = 0.00435M

Molarity of SO3 = 0.0437 / 16.5 = 0.0026M

Molarity of N2O = 0.0222 / 16.5 = 0.0013M

Molarity of N2 = 0.546 / 16.5 = 0.0331M

Keq = [SO3][N2] / [SO2][N2O]

Keq = 0.0026 X 0.0331 / 0.0043 X 0.0013 = 15.39

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