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Q5 10 Points Consider a reaction below: CaCl2 · NH3(s) = CaCl2(s) + NH3(g) A,Hº =...
7 Consider the following reaction at 298 K: NH3(g) +HCI(g)NH4CI(s) Using the thermochemical data at 298 K given below (a) Determine the AH for the reaction. (2 marks) (b) Determine the AG for the reaction and comment on its value. (3 marks) (c) Determine the maximum work done available in the reaction. (3 marks) An equilibrium mixture, consisting of 0.5 atm of NHy(), 0.5 atm of HCKg) and excessive of NH Cl(s), is enclosed in a container at 298 K...
8) Consider the following chemical reaction which is used to produce sulfur trioxide, a precursor in the industrial production of sulfuric acid: 2 SO2(g) + O2(g) → 2 50:(8) Important thermodynamic data associated with this reaction is listed in the table below. Molecule A Hº (kJ/mol) 0 -296.1 -395.2 Sº 0/K mol) 205.0 248.5 256.2 A Gº (kJ/mol) 0 -300.1 -370.4 SO (9) SOS (9) a) Calculate the equilibrium constant (K) for the above reaction at 25 °C. 6 pts)...
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
Consider the following reaction at 25 °C: 5 SO3(g) + 2 NH3(g) → 2 NO(g) + 5 SO2(g) + 3 H2O(g) If AH° = 42.4 kJ./mol and AS° = 562.3 J/ mol•K, estimate the temperature at which this reaction would be at equilibrium assuming that enthalpy and entropy are independent of temperature.
At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches equilibrium when the partial pressures of nitrogen, hydrogen, and ammonia gases are 4.00 atm, 1.00 atm, and 1.05 x 10−2 atm, respectively. Given that the standard enthalpy of the reaction at 400K is DH = -94 kJ/mol, estimate the value of the equilibrium constant KP at 450 K assuming that the standard enthalpy of reaction does not vary significantly with temperature in this temperature...
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 shown below. PbCO3(s) PbO(s) + CO2(g) Calculate the equilibrium pressure of CO2 in the system at the following temperatures. (a) 300°C ____atm (b) 550°C _____atm Note: To find the value of the equilibrium constant at each temperature you must first find the value of G0 at each temperature by using the equation G0 = H0 - TS0 For this reaction the values are H0 = +88.3 kJ/mol and S0= 151.3 J/mol*K
Consider the reaction shown below. PbCO3(s) PbO(s) + CO2(g) Calculate the equilibrium pressure of CO2 in the system at the following temperatures. (a) 240°C ? atm (b) 600°C ? atm Note: To find the value of the equilibrium constant at each temperature you must first find the value of G0 at each temperature by using the equation G0 = H0 - TS0 For this reaction the values are H0 = +88.3 kJ/mol and S0= 151.3 J/mol*K
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