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(a) Consider the following reaction NH4HS(S) NH3g) H2S(g) For this reaction Kp 0.05 atm2 at 20 C. In a particular experiment, 0.06 mole of solid NH4HS is introduced into a 2.4 dm3 flask at 20 '...
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K: NH4HS(s) ->NH3(g) +...
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K: NH4HS(s) ->NH3(g) + H2S(g) Calculate the partial pressure of each gas and the total pressure at equilibrium when 0.581 moles of NH4HS(s) is introduced into a 1.00 L vessel at 298 K. Assume that the volume occupied by the solid is negligible. PNH3 = atm PH2S = atm Ptotal = atm
The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) H3(g) +H2S(g)...
The equilibrium constant, Kc, for the following
reaction is 1.80×10-4 at
298 K.
NH4HS(s) H3(g) +H2S(g) Calculate the equilibrium concentration of H2S when 0.261 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] =
13, 15. The equilibrium constant, K, for the following reaction is 1.80x104 at 298 K. NH4HS(s)...
13, 15.
The equilibrium constant, K, for the following reaction is 1.80x104 at 298 K. NH4HS(s) -NHj(g) + H2S(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.312 mol NH^HS, 1.34x102 M NH3 and 1.34x102 M H2S. If the concentration of NH3(g) is suddenly increased to 2.34x102 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = [H2S]
100 g of solid ammonium hydrogen sulfide (NH4HS) was introduced into an empty 1.0 L reaction...
100 g of solid ammonium hydrogen sulfide (NH4HS) was introduced into an empty 1.0 L reaction vessel. The closed vessel was heated to 300 o C, and the following reaction came to equilibrium: NH4HS(s) ⇌ NH3(g) + H2S(g) At equilibrium, the total pressure inside the reaction vessel was 0.9 atm. Calculate the value of Kp for this reaction.
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) NH3(g) +...
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) NH3(g) + H2S(g) If ΔH° for this reaction is 92.7 kJ, what is the value of Kp at 212 K? Kp =
a) The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g)...
a) The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g) Calculate the equilibrium concentration of H2S when 0.318 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] = _____M b) The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.313 moles of COCl2(g) are introduced into a 1.00 L vessel...
The reaction SO2(g)+2H2S(g) ⇌ 3 S(s)+2H2O(g) is the basis of a suggested method for removal of SO2, a pollutant that...
The reaction SO2(g)+2H2S(g) ⇌ 3 S(s)+2H2O(g) is the basis of a suggested method for removal of SO2, a pollutant that irritates airways causing coughing, from power-plant stack gases. The values below may be helpful when answering questions about the process. Substance ΔG∘f (kJ/mol) ΔH∘f (kJ/mol) H2O(g) −228.6 −241.8 H2O(l) −237.1 −285.8 SO2(g) −300.4 −296.9 SO3(g) −370.4 −395.2 H2S(g) −33.01 −20.17 S(s) 0 0 PART A: Calculate the equilibrium constant Kp for the reaction at a temperature of 298 K. Express...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g)...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) ---------->2HI(g) 1) Calculate the equilibrium concentrations of reactants and product when 0.309 moles of H2 and 0.309 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M? [I2] = M? [HI] = M? 2.The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K: PCl5(g)------->PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a...
1a) Consider the following reaction: 3 C(s) + 4 H2(g) → C3H8(g); ΔH° = –104.7 kJ;...
1a) Consider the following reaction: 3 C(s) + 4 H2(g) → C3H8(g); ΔH° = –104.7 kJ; ΔS° = –287.4 J/K at 298 K What is the equilibrium constant at 298 K for this reaction? Report answer to TWO significant figures. 1b) Τhe enthalpy of vaporization of ammonia is 23.35 kJ/mol at its boiling point (–33 °C). Calculate the value of ΔSsurr when 1.00 mole of ammonia is vaporized at –33 °C and 1.00 atm. Report answer to THREE significant figures.
Write the expressions for Kp for the following reactions: 1. a) 2NH3(g) + Co2(g) N2CH40(s) +...
Write the expressions for Kp for the following reactions: 1. a) 2NH3(g) + Co2(g) N2CH40(s) + H20 (I) b) CuO (s) + H2(g) Cu(l)+H20 (g) 2. At room temperature, a 1.5 L flask contains 3.0 moles of Cl, 0.5 mole of NOCI, and 4.0x10 mole of NO. Calculate Ke at this temperature for the following reaction: 2NO (g) + Cl2(g) 2NOCİ (g) 0.00245 M, does this represent a system at M, [No] 0.2 M and [Ch] If [NOCI] 2.0x 10...
The equilibrium constant, Kc, for the following
reaction is 1.80×10-4 at
298 K.
NH4HS(s) H3(g) +H2S(g) Calculate the equilibrium concentration of H2S when 0.261 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] =
13, 15.
The equilibrium constant, K, for the following reaction is 1.80x104 at 298 K. NH4HS(s) -NHj(g) + H2S(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.312 mol NH^HS, 1.34x102 M NH3 and 1.34x102 M H2S. If the concentration of NH3(g) is suddenly increased to 2.34x102 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = [H2S]
Write the expressions for Kp for the following reactions: 1. a) 2NH3(g) + Co2(g) N2CH40(s) + H20 (I) b) CuO (s) + H2(g) Cu(l)+H20 (g) 2. At room temperature, a 1.5 L flask contains 3.0 moles of Cl, 0.5 mole of NOCI, and 4.0x10 mole of NO. Calculate Ke at this temperature for the following reaction: 2NO (g) + Cl2(g) 2NOCİ (g) 0.00245 M, does this represent a system at M, [No] 0.2 M and [Ch] If [NOCI] 2.0x 10...
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