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) +...
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 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
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, Ky, for the following reaction is 0.110 at 298 K. NH_HS(s) NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 5.50 L container at 298 K contains 2.94 mol of NH_HS(s) and 0.219 mol of NH3(g), the partial pressure of H2S(g) is atm.
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...
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]
The equilibrium constant, K, for the following reaction is 0.186 at 332 K. NH4HS(s) (equilibrium) NH3(g) + H2S(g) An equilibrium mixture in a 16.2 L container at 332 K contains 0.322 mol NH4HS(s), 0.543 M NH3 and 0.343 M H2S. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 8.20 L? [NH3] = M [H2S] = M
6) Distrubuting Equilibrium a) The equilibrium constant, K, for the following reaction is 10.5 at 350 K 2CH2Cl2(g)CH4(g + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.32x10-2 M CH2C2, 0.172 M CH4 and 0.172 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 9.58x102 mol of CH4(g is added to the flask? CH2Cl2l [CH4 [CCI4] b) The equilibrium constant, K, for the...
The equilibrium constant, Kc, for the following reaction is 1.80x104 at 298 K. NH_HS(s) ==NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 5.12 L container at 298 K contains 2.26 mol of NH4HS(s) and 0.282 mol of NH3, the number of moles of H2S present is moles. Submit Answer Retry Entire Group 7 more group attempts remaining
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] =