Consider the reaction: NH3 (g) + HCl (g) → NH4Cl (s) Given the following table of...
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
26. Consider the reaction: (5 pt) NH; (g)+ HCl(g) → NHACI(S) Given the following table of thermodynamic data, Substance AHF (kJ/mol) S /mol.K) NH3 (8) -46.19 1925 HCI (8) -9230 186.69 NH4Cl (s) -3144 946 a. Determine the temperature (in °C) which the reaction is spontaneous Circle one Greater than Less than All None Temp: * Reaction is (non)spontaneous at all temperatures b. Calculate the K for this reaction at 100°C. Answer:
Consider the reaction, NH3 (8) H HC ENH1G(s) Given the following table of thermodynamic data at 298 K: Substana | AH¢{kj/mol | Sº C/K-mol) NH3 (5) 16:19 192.5 HCl (8) 92150 186,69 NHCl (s) 13144 94.6 The value of K for the reaction at 25°C is
step by step for both please T71 pts Consider the reaction: NH, (g) + HCI (9) ► NH,CI (s) Given the following table of thermodynamic data at 298 ok: Substance by admons Imoly NH HCI NHCI 4 6.19 -92.30 -314.4 192.5 186,69 94.6 The value of K for the reaction at 25°C is 150 1.4 x 10 1.1 x10-16 9.3 x1095 8.4 x109 Question 2 1/1 pts The equilibrium constant for the following reaction is 5.0 x 10% at 25°C....
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
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 =
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...
Consider the reaction HCl(g)NH3(g)>NH4C1(s) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.45 moles of HCl(g) react at standard conditions. ASO surroundings J/K Consider the reaction HCl(g)NH3(g)>NH4C1(s) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.45 moles of HCl(g) react at standard conditions. ASO surroundings J/K
Consider the reaction: FeO (s) + Fe (s) + O2(g) → Fe2O3 (s) Given the following table of thermodynamic data at 298 K: Substance ΔHf° (kJ/mol) S° (J/K⋅mol) FeO (s) -271.9 60.75 Fe (s) 0 27.15 O2 (g) 0 205.0 Fe2O3 (s) -822.16 89.96 The value K for the reaction at 25 °C is ________. A.370 B.7.1 x 1085 C.3.8 x 10-14 D.5.9 x 104 E.8.1 x 1019