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

The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 6.76 L container at 548 K contains 3.14 mol of NH4Cl(s) and 0.452 mol of NH3, the number of moles of HCl present is _________moles.

Solutions

Expert Solution

NH4Cl(s) ------------------------------>    NH3(g)   +   HCl(g)

3.14                                        0.452                ? ------------------> at equilibrium

solids doesnot take part in equalibrium constant calculations

K = [NH3][HCl]

5.10 x 10^-6 = 0.452 x [HCl]

[HCl] = 1.13 x 10^-5

moles of HCl = 1.13 x 10^-5

queen_honey_blossom answered 1 year ago
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