Question

Consider the following equilibrium at 1000K:
2SO2 (g) + O2 (g) ¡ê 2SO3 (g)

A study of this system reveals that there are 3.5E-3 moles of sulfur dioxide gas, and 4.8E-3 moles of oxygen gas present in a 11.0L flask at equilibrium. The equilibrium constant for this reaction is 4.2E-3. Calculate the number of moles of SO3(g) in the flask at equilibrium.
oops the equation is actually

2SO2 (g) + O2 (g) yield 2SO3 (g)

the yield part was an arrow facing both directions, not just the product side

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