If an equilibrium mixture of the three compounds in a 7.91 L container at 548 K contains 1.85 mol of NH4Cl(s) and 0.233 mol of NH3(g), the partial pressure of HCl(g) is ______ atm.

Question

The equilibrium constant, K_p , for the following reaction is 1.04×10^-2 at 548 K.

NH₄Cl(s) NH₃(g) + HCl(g)

If an equilibrium mixture of the three compounds in a 7.91 L container at 548 K contains 1.85 mol of NH₄Cl(s) and 0.233 mol of NH₃(g), the partial pressure of HCl(g) is ______ atm.

Answer 1

Kp = (NH3)(HCl) / 1 (solids are not included in the equilibrium expression)

1.04x10^-2 = (2.33)(x)

x = 4.46x10^-3 atm