Calculate the equilibrium constant Kp for the reaction at a temperature of 298 K.
Calculate the equilibrium constant Kp for the reaction at a temperature of 298 K. SO_2 (g) + 2H_2 S (g) reversible 3S...
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...
3. Entropy a. Rank the following systems in order of increasing entropy. i. 1 mol of Ne (g) at 273 K and 20 L ii. 0.5 mol of Ne (g) at 100 K and 20 L ii. 0.5 mol of Ne () at 100 K iv. I mol of CClh (g) at 273 K and 40 L Lowest Entropy: Highest Entropy: The reaction below is the basis of a suggested method for removal of SOs, a pollutant that irritates airways...
The reaction SO2(g)+2H2S(g)⇌3S(s)+2H2O(g) is the basis of a suggested method for removal of SO2 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 Part D...
10a 10b. The equilibrium constant, Kp for the following reaction is 0.110 at 298 K. Calculate Kc for this reaction at this temperature. NH4HS(s) NH3+ H2S(g) Ko The equilibrium constant, Kc, for the following reaction is 5.10x10-6 at 548 K. Calculate Kp for this reaction at this temperature NH4CI(sNH)+ HCI(g) Kp
The equilibrium constant, Kp, for the following reaction is 0.160 at 298 K. Calculate K, for this reaction at this temperature. 2NOBr(g) 2NO(g) + Br2(g) Kc =
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 =
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, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) <----> (arrows both ways) NH3(g) + H2S(g) If ΔH° for this reaction is 92.7 kJ, what is the value of Kp at 391 K? Kp =_______
The equilibrium constant, Kp, for the following reaction is 6.25 at 298 K. 2NO(g) + Br2(g) 2NOBr(g) If ΔH° for this reaction is -16.1 kJ, what is the value of Kp at 187 K? Kp =
The equilibrium constant, Kc, for the following reaction is 1.80*10-4 at 298 K. Calculate Kp for this reaction at this temperature. NH4HS() PNH3(g) + H2S(9) Кр Submit Answer Retry Entire Group 8 more group attempts remaining