Consider the following reaction: NH4Cl(s) -->NH3(g) + HCl(g) If a flask maintained at 560 K contains 0.191 moles of NH4Cl(s) in equilibrium with 3.79×10-2 M NH3(g) and 2.11×10-2 M HCl(g), what is the value of the equilbrium constant at 560 K? K =
Consider the following reaction: NH4Cl(s) -->NH3(g) + HCl(g) If a flask maintained at 560 K contains...
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...
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 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...
Consider the reaction: NH3 (g) + HCl (g) → NH4Cl (s) Given the following table of thermodynamic data at 298 K: Substance! AH/M/mol) I s。(J/K-mol) NH3 g) HCI (g) NHCI)-3144 -46.19 -92.30 192.5 186.69 94.6 The value of K for the reaction at 25 °c is
The equilibrium constant, Kc, for the following reaction is 5.0110 at 514 K. NH4Cl(s) =NH3(g) + HCl(g) Calculate Ke at this temperature for the following reaction: NH3(g) + HCI(g) = NH,Cl(s) K. = ) Submit Answer Retry Entire Group 1 more group attempt remaining
Consider the following reaction and its equilibrium constant K: 3.45 X 10-2 Smol-1: NH3 + HCl ⇌ NH4Cl If concentration for reactants are given as following: [NH3] = 0.20 M; [HCl] = 0.45 M Determine the concentration of NH4Cl in this reaction.
For the reaction HCl(g) + NH3(g) NH4Cl(s) AG° = -77.5 kJ and AS° = -284.8 J/K at 346 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 346 K. The standard enthalpy change for the reaction of 2.15 moles of HCl(g) at this temperature would be kJ. Submit Answer Retry Entire Group 7 more group attempts remaining
Calculate the ΔH0 for the following reaction: NH4Cl(s) → NH3(g) + HCl(g) Given the following standard enthalpies of formation ΔHf0 (298 K, 1 atm) NH3(g) -46.2 kJ mol-1 ; HCl(g) -92.3 kJ mol-1 ; NH4Cl(s) -315.0 kJ mol-1
A 10.0 g sample of NH4Cl(s) is heated in an initially evacuated 5.00 L flask to 900 C. The solid ammonium chloride dissociates into NH3(g) and HCl(g) as products; reaction has Kp= 1.44 at this temperature. A). Calculate the partial pressures of NH3(g) and HCl(g) present at equilibrium. B). Calculate the number of moles of NH3(g) and HCl(g) that will be present in the flask at equilibrium. You may neglect the volume of the solid and assume V=5.00 L.