The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K.
NH4Cl(s) NH3(g) + HCl(g)
If an equilibrium mixture of the three compounds in a 5.41 L container at 548 K contains 1.17 mol of NH4Cl(s) and 0.350 mol of NH3, the number of moles of HCl present is
( ) moles.
The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K.
NH4HS(s) NH3(g) + H2S(g)
If an equilibrium mixture of the three compounds in a 6.48 L container at 298 K contains 3.57 mol of NH4HS(s) and 0.268 mol of NH3, the number of moles of H2S present is
( ) moles.
The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K.
NH4HS(s) NH3(g) + H2S(g)
If an equilibrium mixture of the three compounds in a 7.86 L container at 298 K contains 3.59 mol of NH4HS(s) and 0.459 mol of NH3, the number of moles of H2S present is
( )moles.
The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g)...
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 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.452 moles of NH4Cl(s) are introduced into a 1.00 L vessel at 548 K. [HCl] = _________M -The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2(g) + I2(g) 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.380 moles of H2and 0.380 moles of I2are introduced into a 1.00...
The equilibrium constant, Kc, for the following reaction is 1.80x10+ at 298 K. NH_HS(s) 2NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 6.94 L container at 298 K contains 2.82 mol of NH_HS(s) and 0.209 mol of NH3, the number of moles of H2S present is moles. Submit Answer Retry Entire Group 6 more group attempts remaining
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 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.
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] =
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
The equilibrium constant, K, for the following reaction is 2.57×10-4 at 549 K. NH4Cl(s) NH3(g) + HCl(g) An equilibrium mixture in a 14.3 L container at 549 K contains 0.321 mol NH4Cl(s), 1.97×10-2 M NH3 and 1.30×10-2 M HCl. 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 6.96 L? [NH3] = __________M [HCl] = ___________M
(1). The equilibrium constant, K, for the following reaction is 1.32×10-3 at 565 K. NH4Cl(s) =NH3(g) + HCl(g) An equilibrium mixture in a 10.4 L container at 565 K contains 0.285 mol NH4Cl(s), 4.47×10-2 M NH3 and 2.95×10-2 M HCl. 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 4.25 L? [NH3] = M [HCl] = M
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PC13(g) + Cl2(g) = PC15(g) Calculate the equilibrium concentrations of reactant and products when 0.389 moles of PC13 and 0.389 moles of Cl2 are introduced into a 1.00 L vessel at 500 K [PC13] = [Cl] = [PC15] - The equilibrium constant, Kc, for the following reaction is 5.10x10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.467 moles of NHACI(S)...