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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 0.208 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 3.80×10-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = M [HCl] = M

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Answer #1

[NH3] = 1.62 x 10-3 M

[HCl] = 3.16 x 10-3 M

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