A reaction has ΔS°rxn = +10J/K and an equilibrium constant Kc= 8.0x10^6 at 298 K. Is the reaction exothermic or endothermic?
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A reaction has ΔS°rxn = +10J/K and an equilibrium constant Kc= 8.0x10^6 at 298 K. Is...
A reaction has an equilibrium constant of 8.4 x 10^3 at 298 K. At 800 K, the equilibrium constant is 0.72. Find ∆H°rxn for the reaction. (in kJ)
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) A reaction has an equilibrium constant of Kp=0.280 at 44 ∘C. Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 3.35 kJ -3.35 kJ 0.404 kJ 0.466 kJ B) Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) ΔH= -11.0 kJ; ΔS = -17.4 J/K Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) = -11.0 kJ; = -17.4...
A certain reaction has ΔH°= -19.5 kJ/mol and ΔS°= +42.7 J/mol K a) Is the reaction exothermic or endothermic? b) Does the reaction lead to an increase or decrease in the disorder of the system? c) Calculate ΔG° for the reaction at 298K. d) Is the reaction spontaneous at 298 K under standard conditions?
The equilibrium constant, Kc, for the following reaction is 1.80x10 at 298 K. NH HS(S)N)+HSg) Calculate the equilibrium concentration of HS when 0.529 moles of NH,HS() are introduced into a 1.00 L vessel at 298 K H2S
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, 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...
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, 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. Calculate Kp for this reaction at this temperature. NH4HS() PNH3(g) + H2S(9) Кр Submit Answer Retry Entire Group 8 more group attempts remaining