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1. Ethylene can be formed by cracking of propane: CH CHA+CH. This reaction is carried out...
1. Ethylene can he farmed hy cracking of propane: CHACHA+CH. This reaction is carried out in...
1. Ethylene can he farmed hy cracking of propane: CHACHA+CH. This reaction is carried out in the gas phase. You may assume ideal gas for parts b and c. 68.4 AH (kJ/Llol AG (LJ/mol 52.4 CIL - 103 -23.1 -74.6 -30.5 a. (10%) Use the provided data for 1 bar, 298.15 K) to calculate the exquilibrium constant of this reaction at 298.15 K. b. (10%) Calculate the equilibrium constant of this reaction at 800 K using the shortcut van't Holl...
Predict and calculate the effect of temperature change on an equilibrium system. CHA reacts with CCl4 to form CH2Cl...
Predict and calculate the effect of temperature change on an equilibrium system. CHA reacts with CCl4 to form CH2Cl2. The equilibrium constant, Kp, for this reaction is 9.52x102 at 350 K. CH,(g) +CC1,0)=2CH,C1) The standard enthalpy change for this reaction (AH”) is 18.8 kJ/mol. (a) Predict the effect on the production of CH, Cl, when the temperature of the equilibrium system is increased. production is favored production is disfavored (6) Use the van't Hoff equation to estimate the equilibrium constant...
thermodynamics 2 Cumene (isopropyl benzene) and propylene are reacted together with 50% excess cumene to form...
thermodynamics 2
Cumene (isopropyl benzene) and propylene are reacted together with 50% excess cumene to form diisopropyl benzene. The propylene source includes propane in a 0.10:1 propane:propylene ratio. The propane is inert at the conditions of interest. Write a balanced stoichiometric equation for this reaction. Estimate the equilibrium constant (Ka) at 680 K and 90 bar) according to the shortcut van't Hoff equation. Energy of formation data: Species dH(f,298), kJ/mol dG(f,298), kJ/mol Propylene 19.71 62.14 Cumene 3.93 137.15 147.83 Diisopropyl...
Standard conditions 298.15 K (25 °C) and 1 bar. Thermodynamic Data Conversions Factors I cal 4.18...
Standard conditions 298.15 K (25 °C) and 1 bar. Thermodynamic Data Conversions Factors I cal 4.184 J 1 bar 0.10 J cm 1 atm 1.01325 bar 1 cm 0.10 J bar 0°C 273.15K Species/ Phase AHP J mol) MnCOs) Mn2 mo K) V° (cm mo) -894.1 -220.75 -167.159 -393.509 167.159 -285.83 85.8 73.6 56.5 213.79 56.5 69.91 31.073 21.0 17.3 24.7892 L mol 17.3 18.068 Cl CO2() Constants HCI R 8.3145 J mol! K-1 H:Op Continuing with the carbonate reaction...
please show how you got the answer For the gas-phase reaction A=B, you make a series...
please show how you got the answer
For the gas-phase reaction A=B, you make a series of measurements of the equilibrium constant at constant pressure over a range of temperatures. With this data, you construct the following van't Hoff plot: 14, 12 o slope - 5 x 103 K o 10 8 In KP 6 2 AB 1.5 3 4 3.5 17 T (K) 4.5 x 103 When you fit the data to a straight line, you find a slope...
Standard conditions 298.15 K (25 °C) and 1 bar. Thermodynamic Data Conversions Factors I cal 4.184...
Standard conditions 298.15 K (25 °C) and 1 bar. Thermodynamic Data Conversions Factors I cal 4.184 J 1 bar 0.10 J cm 1 atm 1.01325 bar 1 cm 0.10 J bar 0°C 273.15K Species/ Phase AHP J mol) MnCOs) Mn2 mo K) V° (cm mo) -894.1 -220.75 -167.159 -393.509 167.159 -285.83 85.8 73.6 56.5 213.79 56.5 69.91 31.073 21.0 17.3 24.7892 L mol 17.3 18.068 Cl CO2() Constants HCI R 8.3145 J mol! K-1 H:Op Continuing with the carbonate reaction...
A coal gasifier produces a mixture of 1 mol/s of CO and 2 mol/s of H2....
A coal gasifier produces a mixture of 1 mol/s of CO and 2 mol/s of H2. This is fed to a catalytic converter to produce methane, the gas phase reaction is CO + 3H2-CH4 +H20 The reactor operates at 600°K and 600 kPa. a) Find the equilibrium constant for the above reaction at standard conditions b) Find the equilibrium constant at operating conditions c) Find the outlet stream composition at operating conditions 5 Marks 5 Marks 5 Marks H20 -241.8...
4. The gas-phase dehydrogenation of propanol (A) to yield propionaldehyde (B) is in equilibrium at 230°C. Standard thermodynamic data for the reaction species at 298 K are: Propanol: Propionaldehyde...
4. The gas-phase dehydrogenation of propanol (A) to yield propionaldehyde (B) is in equilibrium at 230°C. Standard thermodynamic data for the reaction species at 298 K are: Propanol: Propionaldehyde : H.,--186 k/moi s'u-304.40 J/(mol K) Dihydrogen: H A -256 kJ/molSA 322.49 J/(mol K) Soc 130.68 J/(mol K) ) (4 points) Evaluate the standard enthalpy change of reaction (AH)at 298 K. ii (6 points Calculate the equilibrium constant at 298 K ) (8 points) Determine the equilibrium constant for this reaction...
2. We wish to produce formaldehyde by the gas-phase pyrolysis of methanol, CH,OH (8)=CH,0 (8)+H, ()...
2. We wish to produce formaldehyde by the gas-phase pyrolysis of methanol, CH,OH (8)=CH,0 (8)+H, () The following table provides AH 295, AGM298 and C/R = A+BT +CT2 + DT ?, T'in K, for the species involved in the pyrolysis reaction. Species AH 29(J/mol) AG298 (J/mol) A 10B 10°C 10 D 0 CH,OH CH,0 H -200660 -108570 -161960 -102530 2.211 2.264 3.249 12.216 7.022 0.422 -3.450 -1.877 0 0.083 0 0 0 (a) (15 pts) Calculate heat of reaction and...
1. (14 pts) Consider the following unbalanced gas-phase exothermic reaction, N2 + O2 = NO2 This...
1. (14 pts) Consider the following unbalanced gas-phase exothermic reaction, N2 + O2 = NO2 This is a reaction involved in the production of smog. The heat of formation of NO2 from the elements is A He = 33.18 kJ/mol. This is an endothermic process. The 4, Gof NO2 is 51.31 kJ/mol. a) Balance the reaction. b) Calculate the equilibrium constant at room temperature (300 K). c) If we assume that in our atmosphere the partial pressure of oxygen is...
1. Ethylene can he farmed hy cracking of propane: CHACHA+CH. This reaction is carried out in the gas phase. You may assume ideal gas for parts b and c. 68.4 AH (kJ/Llol AG (LJ/mol 52.4 CIL - 103 -23.1 -74.6 -30.5 a. (10%) Use the provided data for 1 bar, 298.15 K) to calculate the exquilibrium constant of this reaction at 298.15 K. b. (10%) Calculate the equilibrium constant of this reaction at 800 K using the shortcut van't Holl...
Predict and calculate the effect of temperature change on an equilibrium system. CHA reacts with CCl4 to form CH2Cl2. The equilibrium constant, Kp, for this reaction is 9.52x102 at 350 K. CH,(g) +CC1,0)=2CH,C1) The standard enthalpy change for this reaction (AH”) is 18.8 kJ/mol. (a) Predict the effect on the production of CH, Cl, when the temperature of the equilibrium system is increased. production is favored production is disfavored (6) Use the van't Hoff equation to estimate the equilibrium constant...
thermodynamics 2
Cumene (isopropyl benzene) and propylene are reacted together with 50% excess cumene to form diisopropyl benzene. The propylene source includes propane in a 0.10:1 propane:propylene ratio. The propane is inert at the conditions of interest. Write a balanced stoichiometric equation for this reaction. Estimate the equilibrium constant (Ka) at 680 K and 90 bar) according to the shortcut van't Hoff equation. Energy of formation data: Species dH(f,298), kJ/mol dG(f,298), kJ/mol Propylene 19.71 62.14 Cumene 3.93 137.15 147.83 Diisopropyl...
Standard conditions 298.15 K (25 °C) and 1 bar. Thermodynamic Data Conversions Factors I cal 4.184 J 1 bar 0.10 J cm 1 atm 1.01325 bar 1 cm 0.10 J bar 0°C 273.15K Species/ Phase AHP J mol) MnCOs) Mn2 mo K) V° (cm mo) -894.1 -220.75 -167.159 -393.509 167.159 -285.83 85.8 73.6 56.5 213.79 56.5 69.91 31.073 21.0 17.3 24.7892 L mol 17.3 18.068 Cl CO2() Constants HCI R 8.3145 J mol! K-1 H:Op Continuing with the carbonate reaction...
please show how you got the answer
For the gas-phase reaction A=B, you make a series of measurements of the equilibrium constant at constant pressure over a range of temperatures. With this data, you construct the following van't Hoff plot: 14, 12 o slope - 5 x 103 K o 10 8 In KP 6 2 AB 1.5 3 4 3.5 17 T (K) 4.5 x 103 When you fit the data to a straight line, you find a slope...
Standard conditions 298.15 K (25 °C) and 1 bar. Thermodynamic Data Conversions Factors I cal 4.184 J 1 bar 0.10 J cm 1 atm 1.01325 bar 1 cm 0.10 J bar 0°C 273.15K Species/ Phase AHP J mol) MnCOs) Mn2 mo K) V° (cm mo) -894.1 -220.75 -167.159 -393.509 167.159 -285.83 85.8 73.6 56.5 213.79 56.5 69.91 31.073 21.0 17.3 24.7892 L mol 17.3 18.068 Cl CO2() Constants HCI R 8.3145 J mol! K-1 H:Op Continuing with the carbonate reaction...
A coal gasifier produces a mixture of 1 mol/s of CO and 2 mol/s of H2. This is fed to a catalytic converter to produce methane, the gas phase reaction is CO + 3H2-CH4 +H20 The reactor operates at 600°K and 600 kPa. a) Find the equilibrium constant for the above reaction at standard conditions b) Find the equilibrium constant at operating conditions c) Find the outlet stream composition at operating conditions 5 Marks 5 Marks 5 Marks H20 -241.8...
4. The gas-phase dehydrogenation of propanol (A) to yield propionaldehyde (B) is in equilibrium at 230°C. Standard thermodynamic data for the reaction species at 298 K are: Propanol: Propionaldehyde : H.,--186 k/moi s'u-304.40 J/(mol K) Dihydrogen: H A -256 kJ/molSA 322.49 J/(mol K) Soc 130.68 J/(mol K) ) (4 points) Evaluate the standard enthalpy change of reaction (AH)at 298 K. ii (6 points Calculate the equilibrium constant at 298 K ) (8 points) Determine the equilibrium constant for this reaction...
2. We wish to produce formaldehyde by the gas-phase pyrolysis of methanol, CH,OH (8)=CH,0 (8)+H, () The following table provides AH 295, AGM298 and C/R = A+BT +CT2 + DT ?, T'in K, for the species involved in the pyrolysis reaction. Species AH 29(J/mol) AG298 (J/mol) A 10B 10°C 10 D 0 CH,OH CH,0 H -200660 -108570 -161960 -102530 2.211 2.264 3.249 12.216 7.022 0.422 -3.450 -1.877 0 0.083 0 0 0 (a) (15 pts) Calculate heat of reaction and...
1. (14 pts) Consider the following unbalanced gas-phase exothermic reaction, N2 + O2 = NO2 This is a reaction involved in the production of smog. The heat of formation of NO2 from the elements is A He = 33.18 kJ/mol. This is an endothermic process. The 4, Gof NO2 is 51.31 kJ/mol. a) Balance the reaction. b) Calculate the equilibrium constant at room temperature (300 K). c) If we assume that in our atmosphere the partial pressure of oxygen is...
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