At a certain temperature, 5.00 mol of sulfur trioxide, SO3 is placed into a 5.00L container and allowed to decompos according to the reaction 2SO32SO2 + O2. At equilibrium, 3.00 mol of sulfur dioxide, SO2 is present. Calculate the equilibrium concentrations of O2, SO2, and SO3 Help?!?!

Question

At a certain temperature, 5.00 mol of sulfur trioxide, SO3 is placed into a 5.00L container and allowed to decompos according to the reaction 2SO3<-->2SO2 + O2. At equilibrium, 3.00 mol of sulfur dioxide, SO2 is present.

Calculate the equilibrium concentrations of O2, SO2, and SO3

Help?!?!

jfraser · Answer

You know that the reaction started with 5mol of SO3. You also know that 3mol of SO2 are present at equilibrium. In order to form those 3mol of SO2, 3mol of SO3 has to be used up. So out of the 5 mol, 3 were used to form the SO2. The remaining SO3 is still tehre. The oxygen is formed HALF AS MUCH so the SO2 is, because of the stoichiometric ratio. So forming 3mol of SO2 will form 1.5mol of O2. This all belongs in an ICE table or RICE box, but I can't do tables here. If there's a way, I'd love to know

mos1635 · Answer

2SO3<-->2SO2 + O2
5mol         0 mol     0mol
-3mol        +3mol    +1.5mol
2mol           3mol         1.5mol

[each]=n(each)/V

anonymous · Answer

Thank you! :)