What Are the New Equilibrium Concentrations After Removing 1.0 mol/L of SO2?

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The discussion revolves around calculating the new equilibrium concentrations after removing 1.0 mol/L of SO2 from a reaction mixture of O2 and SO2 forming SO3. Initially, 8.0 moles of O2 and 10.0 moles of SO2 are present in a 2.0L container, with 3.0 moles/L of SO3 remaining at equilibrium. Participants suggest using an ICE table to determine the initial concentrations and the shifts in equilibrium after the removal of SO2. The need for calculating the equilibrium constant is also mentioned, emphasizing the importance of stoichiometry in these calculations. The thread highlights the challenges faced by students in understanding equilibrium shifts and concentration calculations.
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8.0 mole of O2(g) is mixed with 10.0 moles of SO2(g) in a 2.0L container forming SO3(g). If 3.0 moles/L of SO3(g) remains at equilibrium. 1.0 mol/L of SO2(g) is removed from the equilibrium, calculate the new eq'm [ ]'s.So I make the rice table

3O2(g) + SO2(g) <--> 2SO3(g)
r 3 ... : ... 1 ... : 2
4.0M ... 5.0M ... 0M (shift right)
c -3x ... -3x ... +2x
e 4.0 -3x ... 5.0-3x ... 2xwhat do I do now?
 
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Guise I need help on this homework question please, it's really bothering me and I am stuck.
 
What were the concentrations of all gases before SO2 was removed? Can you calculate them from the stoichiometry? After they are calculated - can you use them to calculate equilibrium constant?

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