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The equilibrium constant, K, for the following reaction is 5.10×10-6 at 548 K.
NH4Cl(s) <-----> NH3(g) + HCl(g)
An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.252 mol NH4Cl, 2.26×10-3M NH3 and 2.26×10-3 M HCl. If the concentration of NH3(g) is suddenly increased to 3.91×10-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished?
[NH3] = ? M
[HCl] = ? M
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