Gen Chm II

Determine the pressure-based Keq for the reaction:
2SO2(g) + O2(g)<--->2SO3(g)

given that 1.00×10−2 moles of SO2 and 2.00×10−2 moles of O2 were initially placed in a 2.00 L reaction chamber. The chamber contained 7.5×10−3 moles of SO3 when equilibrium was established at 727 °C. Since you need to calculate the pressure-based equilibrium constant, you will need to use the ideal gas equation (PV=nRT) to convert the moles of gas into pressure with units of atmospheres. (remember that one formulation of R is 0.0821 L·atm/mol·K)

Kind of overwelmed me, thank you for your help

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1. I think the easiest thing to do is use mols to begin and convert to pressure later.
..........2SO2 + O2 ==> 2SO3
I.........0.01..0.02.....0
C.........-2x....-x.....2x
E.......0.01-2x..0.02-x..2x

The problem tells you that E mols sO3 = 0.0075 so 2x = 0.0075 which makes x = 0.00375
That means mols sO2 = 0.01-2x
and mols O2 = 0.02-x
and mols SO3 = 0.0075
Now convert each of those to pressures in atmospheres using PV = nRT. You know n, R, T is 727+273 = 1000 and V is 2L
Substitute p into
Kp = pSO3^2/pSO2^2*pO2 and solve for Kp.

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posted by DrBob222

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