At a certain temperature, the equilibrium constant for the following chemical?

Question

At a certain temperature, the equilibrium constant for the following chemical equation is 3.20. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.86 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibrium.
 SO2+NO2<-->SO3+NO
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_______mol of NO2 (g)
 i got 0.51 but its saying its wrong that :The number of gaseous products equals the number of gaseous reactants and so Kp = Kc = 3.20. This means that instead of having to use concentrations or pressures, you can leave the quantities in moles in the K expression.

? · Answer

use an ICE table, this gives

K = (x mol SO3 . x mol NO)/((2.86 - x) mol SO2 . (I - x) mol NO2) = 3.20

now x = 1.30 so solve for I, the initial mol NO2 needed

akihiko · Answer

The equlibrium constant is expressed by concentration or pressure unit, not mole.

At a certain temperature, the equilibrium constant for the following chemical?

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