Consider the decomposition of Baco3(s) into Ba) and Co2(g). What is the eqilibrium partial pressure (in...
Consider the following reaction occurring at 298 K: BaCO3(s)⇌BaO(s)+CO2(g) Part A Show that the reaction is not spontaneous under standard conditions by calculating ΔG∘rxn. ΔG∘rxn =? Part B If BaCO3 is placed in an evacuated flask, what partial pressure of CO2 will be present when the reaction reaches equilibrium? P=? Part C What temperature is required to produce a carbon dioxide partial pressure of 1.0 atm? T=?
5. What is AH for BaCO3 (5) → BaO (5)+ CO2 (g) Given reactions 2 Ba (s)+02 g) + 2 BaO (s) Ba (s) + CO2 (g) + 1/2O2 (g) → BaCO3 (g) AH = -1106.0 kJ AH = -822.0 kJ
Substance BaCO3(s) | BaO(s) CO2(g) BaCO3(s) = Bao(s) + CO2(g) A.HⓇ/kJ mol -1213.0 -548.0 -393.5 Sº / 1 mol K- 112.1 72.1 213.8 a. Using the information in the table above, show that the reaction is not spontaneous under standard conditions by calculating 4,Gº. {5 marks) b. If Baco, is placed in an evacuated flask, what partial pressure of CO2 will be present when the reaction reaches equilibrium? (3 marks) c. Can the reaction be made more spontaneous by an...
Consider the heterogeneous equilibrium process: C(s) + CO2(g) ⇆ 2CO(g) At 700°C, the total pressure of the system is found to be 1.50 atm. If the equilibrium constant (KP) is 1.52, calculate the equilibrium partial pressures of CO and CO2.
A container encloses 33.1 g of CO2(g). The partial pressure of CO2 is 2.89 atm and the volume of the container is 31.5 L. What is the average, or root mean square, speed (in m/s) of the CO2 molecules in this container?
If 1.5g of ammonium carbamate is placed in a 1.50L flask and
some CO2 is added so that the partial pressure of CO2 at
equilibrium is 1.5atm, what is the partial pressure of NH3 when the
system comes at equilibrium at 25 degrees?
The final answer should be 0.0214barr or atm, please show your
work, thank you.
Ammonium carbamate, NH4CO2NH2, dissociates according to the exothermic reaction: 4.62 × 10-4 at 25°C NH,co2NH2 (s) 2 NH2(g) + CO2(g) Kp
Ammonium carbamate,...
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
9. Consider the following reaction: inputted, <GO CaO(s) + CO2(g) - CaCO3(s); AG° = -130.9 kJ at 298 K At what partial pressure of CO2(g) will the reaction no longer be spontaneous at 298 K? (R- 0.0821 L.atm/(K.mol) = 8.31 J/(K.mol)) a. 1.59 x 108 atm b. 1.00 atm c. 6.28 x 10 atm d. 8.77 x 1022 atm e. 1.14 x 10-23 atm
Consider the following reaction: SiCl4(g) ⇌ Si(s) + 2Cl2(g) The initial partial pressure of SiCl4 is 1.00 atm. At equilibrium, the total pressure is 1.35 atm. Calculate Kp for this reaction. Report your answer to the correct number of significant figures.
The solubility of CO2 in water exposed to the atmosphere, where the partial pressure of CO2 is 3.87 10 atm, is 1.32 * 10 M. At the same temperature, what would be the solubility of pressurized CO2, at a pressure of 68 atm? a. 5.09 x 10*M b. 2.32 M C. 1920 M d. 4310 M How many mL of a 0.575 M glucose solution (MW=184 g/mol) would be needed to make 350 ml of a 0.320 M glucose solution?...