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The equilibrium constant, K, for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) --> NH3(g)...

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 0.255 mol NH4Cl, 2.26×10-3 M NH3 and 2.26×10-3 M HCl. If the concentration of HCl(g) is suddenly increased to 3.55×10-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished?

[NH3] = M

[HCl] = M

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