Excess solid ammonium chloride, NH4Cl (s), decomposes into hydrogen, nitrogen an

Question

Excess solid ammonium chloride, NH4Cl (s), decomposes into hydrogen, nitrogen and chlorine gases.. If excess NH4Cl (s) is initially present with 1.00 atm N2 (g), 1.5 atm Cl2 (g) , and zero hydrogen, find the equilibrium partial pressures (in atm) of all three gaseous products. ( Kp = .640 ) First, write the balanced chemical equation using whole number coefficients; then construct a reaction table to solve. 1) the approximation method (and 5% check) 2) successive approximation method, which provides the precisely correct answer. I have gotten to here: 2NH4Cl(s) <-----> N2(g) + 4H2(g) + Cl2(g) Kp = PN2*PCl2*(PH2)4 Let at eqb., PN2 = (1 + x) atm ; PCl2 = (1.5 + x) atm & PH2 = 4x atm Thus, Kp = (4x)4*(1+x)*(1.5+x) or, 0.64 = (4x)4*(1+x)*(1.5+x) What I need is detailed help for #1 and 2 so I can figure out where I am going wrong.

Explanation / Answer

2 NH4Cl(s) <-----> N2(g) + 4H2(g) + Cl2(g)

initial partial pressure: 2 moles 1 atm 0 1.5 atm

eqlb partial pressure: 2-x moles 1+x 4x   1.5+x

Kp = P N2*P Cl2*(P H2)4

0.64 =(1+x)*(1.5+x) * (4x)4

approx

0.64 = 1*1.5*256x4

x4 = 0.0016

x = 0.0104

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