A. Ammonium hydrogen sulfide decomposes according to the following reaction, for

Question

A. Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp .11 at 2500C. NHHS(s) H2S(g) NH3(g If 55.0 g of the solid is placed in a sealed 5.0L container, what is the partial pressure of ammonia at equilibrium? B. The key process in a blast furnace during the production of iron is the reaction of Fe2O3 and carbon to form Fe and CO. 2Fe2O3(s) 3C 4Fe(s) 3CO mo mio 87.4 Fe20, 825.5 5.686 COgr. 27.3 Fe(s) 3935 213.7 CO2 (g) a) Given the information in the table above, calculate AH0 at 298 K in kJ. b) Calculate ASO at 298 K in J/K. Calculate AG at 298 K in kJ

Explanation / Answer

A. moles of NH4HS = 55/51.1 = 1.08 mols

initial pressure = 1.08 x 0.08205 x (273 + 250)/5 = 9.3 atm

let x be the change at equilibrium

11 = x^2/(9.3 - x)

x^2 + 11x - 102.3 = 0

x = 6.0 atm

Partia pressure of NH3 at equilibrium = 6.0 atm

B.

a) dHo = (3 x -393.5) - (2 x -825.5) = 470.5 kJ

b) dSo = (4 x 27.3 + 3 x 213.7) - (2 x 87.4 + 3 x 5.686) = 558.44 J/K

c) dGo = dHo - TdSo = 304.08 kJ

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