(1-16)Chemistry - Science

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

The reaction vessel is charged initially with all four gases, each at a pressure of 0.5 atm. After equilibrium is achieved, the partial pressure of SO3 will be:
a) 0.250 atm
b) 0.500 atm
c) 0.750 atm
d) 0.900 atm
e) none of these

asked by Ana
  1. First you must determine which way the reaction will shift to reach equilibrium.
    Q = (SO3)(NO)/(NO2)(SO2) = (0.5*0.5/0.5*0.5) = 1. With K = 9 that means products are too small and reactants too large so the rxn must shift to the right to reach equilibrium.
    .....SO2(g) + NO2(g) ==> SO3(g) + NO(g)
    I...0.5.......0.5.........0.5.....0.5
    C.....-x......-x..........x.......x
    E...0.5-x...0.5-x........0.5+x...0.5+x

    Substitute into Keq an solve for x, then evaluate each constituent.

    posted by DrBob222

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