a.) Consider the following equilibrium at 395K NH 4 HS(s) = NH 3 (g) +H 2 S (g)
ID: 682530 • Letter: A
Question
a.) Consider the following equilibrium at 395K NH4HS(s) = NH3(g) +H2S (g) The partial pressure of each gas at equilibrium is .0265 atm.Calculate Kp and Kc for the reaction. b.) The equilibrium constant Kc for thereaction N2 (g) + 3 H2(g) = 2 NH3(g) 3.5 x 108 at 25oC. Determinr Kc at 25oC for thereaction 2/3 NH3(g) + 1/3N2(g) + H2(g) c.) The equilibrium constant Kp for thereaction SO2(g) + 1/2 O2 (g) =SO3(g) is 2.37 x 102 at 350oC. DetermineKp at 350oC for the reaction 2SO2 (g) + O2 (g) = 2 SO3 (g) a.) Consider the following equilibrium at 395K NH4HS(s) = NH3(g) +H2S (g) The partial pressure of each gas at equilibrium is .0265 atm.Calculate Kp and Kc for the reaction. b.) The equilibrium constant Kc for thereaction N2 (g) + 3 H2(g) = 2 NH3(g) 3.5 x 108 at 25oC. Determinr Kc at 25oC for thereaction 2/3 NH3(g) + 1/3N2(g) + H2(g) c.) The equilibrium constant Kp for thereaction SO2(g) + 1/2 O2 (g) =SO3(g) is 2.37 x 102 at 350oC. DetermineKp at 350oC for the reaction 2SO2 (g) + O2 (g) = 2 SO3 (g)Explanation / Answer
a) NH4HS(s) = NH3(g) +H2S (g) Kp = PNH3 * PH2S / PNH4HS =0.0265atm * 0.0265atm / 0.0265 atm = 0.0265 Kp = Kc * (RT)n 0.0265= Kc * ( 8.314 J/K.mol * 395K )1 Kc = 8.069 x 10-6 b) N2 (g) + 3H2(g) = 2 NH3 (g) Kc = [NH3]2 /[H2]3 * [N2] = 3.5 x 108 2/3 NH3(g) = 1/3 N2(g) +H2(g) Kc1 = [N2]1/3 *[H2] / [NH3]2/3 = ( 1 / Kc )1/3 = (1 / 3.5 x 108)1/3 = 0.658 x 10-8/3 c) SO2(g) + 1/2O2 (g) = SO3(g) Kc = [SO3 ] / [O2]1/2* [SO2]2 2SO2 (g) + O2 (g) = 2 SO3 (g) Kc1 = [SO3]2 / [O2] *[SO2]2 = (Kc)2 = (2.37 x 102 )2 = 5.616 x 104 = 5.616 x 104Related Questions
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