26. Consider the reaction: (5 pt) NH; (g)+ HCl(g) → NHACI(S) Given the following table of...
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
step by step please TT1 pts Consider the reaction: NHą (g) + HCI (g) → NH,CI (s) Given the following table of thermodynamic data at 298 ok: Substance (kJ/mol S(J/mol) NH |-46.19 192.5 HCI -92.30 186.69 NHCI -314.4 94.6 The value of K for the reaction at 25 °C is 150 1.4 x108 1.1 x10-16 9.3 Ⓡ1015 8.4 x104
Consider the reaction: 2NO(g) + C12(8) + 2NOCI(g) Given the following table of thermodynamic data, AHF (kJ/mol) Substance NO (8) Cl2 (8) NOCI (8) 90.3 0 sº (l/mol.K) 210.7 223.0 261.6 51.7 Calculate Ahºrxn and Asºrxn and determine the temperature at which the reaction switches from being spontaneous to being non- spontaneous.
Consider the reaction: 2NO(g) + Cl2(g) → 2NOCI(g) Given the following table of thermodynamic data, Substance NO (g) Cl2(g) NOCI (g) AH (kJ/mol) 90.3 0 sº (/mol.K) 210.7 223.0 51.7 261.6 Calculate Ahºrxn and AS rxn and determine the temperature at which the reaction switches from being spontaneous to being non-spontaneous.
Please show steps. Thank you. Consider the reaction: NH3 (g) + HCl (g) NHỊd(s). Given the following table of thermodynamic data at 298 K: Substance Hitmol) | SPIK.mol) HGS The siue ot k for the reaction at 25 C us
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
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
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 =
NH,(8) + HCl(g) NH,Cl(s) A 6.55 g sample of NH, gas and a 6.55 g sample of HCl gas are mixed in a 1.50 L flask at 25°C. Identify the limiting reagent. HCI ONH,CI Ο ΝΗ, How many grams of NH CI will be formed by this reaction? mass: What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH, CI produced by the reaction.
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)...