Consider the reaction:
SO2 (g) + NO2 (g) SO3 (g) + NO (g)
At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00
If the reaction vessel is instead charged initially with SO3(g) and NO(g), each at a partial pressure of 0.500 atm, the partial pressure of SO2(g) at equilibrium will be:
a) 0.050 atm
b) 0.125 atm
c) 0.250 atm
d) 0.375 atm
e) none of these
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Isn't this done the same way except you know the reaction must shift to the left to reach equilibrium?
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