Calculate the equilibrium constant for the hydration reaction of ethylene with water to produce ethanol at...
Calculate the equilibrium constant for the hydration reaction of ethylene with water to produce ethanol at a temperature of 280 K and a pressure of .8 atm
C2H4(g) + H2O(g) ? C2H5OH(g)
?H?rxn = -47.8 kJ Kc = 9 x 103 at 600K
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Calculate the equilibrium constant for the hydration reaction of
ethylene with water to produce ethanol at...
1. Ethanol is produced by the hydration of ethylene. Some of the ethanol product is converted...
1. Ethanol is produced by the hydration of ethylene. Some of the ethanol product is converted in an undesired side reaction to diethyl ether and water. C2H4 (g) + H20 (1) → C2H5OH (1) 2 C2H5OH (1) → (C2H5)20 (1) + H20 (1) The feeds to the reactor are ethylene gas and liquid water, each @ 25°C, 1 atm. A sample of the reactor effluent is analyzed and found to be 15°C and contain 43.3 mol% ethylene (g), 2.5% ethanol...
ethanol(the desired product) is produced commercially by the hydration of ethylene: C2H4 + H2O −→ C2H5OH...
ethanol(the desired product) is produced commercially by the hydration of ethylene: C2H4 + H2O −→ C2H5OH Some of the product is converted to the undesired product diethyl ether by the side reaction C2H5OH −→ (C2H5)2O + H2O The feed to the reactor contains 53.7% mole C2H4 ,36.7% H2O,and the balance is non-reactive inert gases.these intert gases do not resct as they pass through the reactor. an ethylene conversion 5% and an efficiency as defined in your class notes of 90%...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + O2(g) → CO2(g) + H2O(g) ΔH°rxn = ? (Points : 1) -1.24 × 103 kJ/mol +1.24 × 103 kJ/mol -8.09 × 103 kJ/mol -9.55 × 103 kJ/mol...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + O2(g) → CO2(g) + H2O(g) ΔH°rxn = ? (Points : 1) -1.24 × 103 kJ/mol +1.24 × 103 kJ/mol -8.09 × 103 kJ/mol -9.55 × 103 kJ/mol...
Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium...
Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g). C2H4(g) + H2O(g) ⇌ C2H5OH(g) Kc = 9.0 × 104 [C2H4]eq = 0.95 M [C2H5OH]eq = 5.03 M A. A) 9.9 × 10-7 M B. B) 80.0 M C. C) 5.9 x 10-5 D. D) 1.68 M E. E) 0.021 M F. F) none of these
Page 4 8. A check of the formulas of ethylene, water, that the reaction, C, H. (g) + HO(g) -> C215 to occur under...
Page 4 8. A check of the formulas of ethylene, water, that the reaction, C, H. (g) + HO(g) -> C215 to occur under the correct conditions. Mike G. says it's just a matter of t reactor temperature, and pressure. U below, what is the calculated value of AHO reaction? I ethylene, water, and ethanol suggests 9) + H2O(g) -> C2H5OH(1) could be made correct conditions. This is a wild idea, but just a matter of the right catalyst combination,...
8. Ethanol (C2H5OH) is synthesized for industrial use by the following reaction, carried out at very...
8. Ethanol (C2H5OH) is synthesized for industrial use by the following reaction, carried out at very high pressure. C2H4 (g) + H2O(g) - C2H5OH (1) What is the maximum amount, in kg. of ethanol that can be produced when 1.45 kg of ethylene (C2H4) and 0.0433 kg of steam are placed into the reaction vessel? How many kg of excess reactant will be left over?
True or False t. For an exothermic reaction, the equilibrium constant, Kc, becomes smaller as the...
True or False
t. For an exothermic reaction, the equilibrium constant, Kc, becomes smaller as the temperature increases and larger as the temperature decreases. u. The gas-phase equilibrium shown below is used to produce ammonia, NH3, for commercial applications. The NH3 yield can be increased by decreasing the temperature, increasing the pressure, and removing some NH; from the mixture. N2(g) + 3H2(g) - 2NH3() AH = -94 kJ. v. For the gas-phase equilibrium described above (see problemlu), an increase in...
19) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the...
19) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g). C2H4(8) + H2O(g) - C2H5OH(g) Kc = 9.0 x 103 (C2H4leq=0.015 M [C2H5OHleq=1.69 M A) 1.0 M B) 9.9 x 10-7 M C) 0.013 M D) 1.68 M E) 80.M 20) Consider the following reaction at equilibrium. What effect will increasing the volume of the reactic mixture have on the system? 20) 2 H2S(8) + 3 O2(g) + 2 H2O(g)...
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction...
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) The bomb had a heat capacity of 500 J/K, and the calorimeter contained 610 g of water. Burning 4.50 g of ethanol, C2H5OH(L) resulted in a rise in temperature from 16.5 °C to 20.9 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184...
1. Ethanol is produced by the hydration of ethylene. Some of the ethanol product is converted in an undesired side reaction to diethyl ether and water. C2H4 (g) + H20 (1) → C2H5OH (1) 2 C2H5OH (1) → (C2H5)20 (1) + H20 (1) The feeds to the reactor are ethylene gas and liquid water, each @ 25°C, 1 atm. A sample of the reactor effluent is analyzed and found to be 15°C and contain 43.3 mol% ethylene (g), 2.5% ethanol...
Page 4 8. A check of the formulas of ethylene, water, that the reaction, C, H. (g) + HO(g) -> C215 to occur under the correct conditions. Mike G. says it's just a matter of t reactor temperature, and pressure. U below, what is the calculated value of AHO reaction? I ethylene, water, and ethanol suggests 9) + H2O(g) -> C2H5OH(1) could be made correct conditions. This is a wild idea, but just a matter of the right catalyst combination,...
8. Ethanol (C2H5OH) is synthesized for industrial use by the following reaction, carried out at very high pressure. C2H4 (g) + H2O(g) - C2H5OH (1) What is the maximum amount, in kg. of ethanol that can be produced when 1.45 kg of ethylene (C2H4) and 0.0433 kg of steam are placed into the reaction vessel? How many kg of excess reactant will be left over?
True or False
t. For an exothermic reaction, the equilibrium constant, Kc, becomes smaller as the temperature increases and larger as the temperature decreases. u. The gas-phase equilibrium shown below is used to produce ammonia, NH3, for commercial applications. The NH3 yield can be increased by decreasing the temperature, increasing the pressure, and removing some NH; from the mixture. N2(g) + 3H2(g) - 2NH3() AH = -94 kJ. v. For the gas-phase equilibrium described above (see problemlu), an increase in...
19) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g). C2H4(8) + H2O(g) - C2H5OH(g) Kc = 9.0 x 103 (C2H4leq=0.015 M [C2H5OHleq=1.69 M A) 1.0 M B) 9.9 x 10-7 M C) 0.013 M D) 1.68 M E) 80.M 20) Consider the following reaction at equilibrium. What effect will increasing the volume of the reactic mixture have on the system? 20) 2 H2S(8) + 3 O2(g) + 2 H2O(g)...
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) The bomb had a heat capacity of 500 J/K, and the calorimeter contained 610 g of water. Burning 4.50 g of ethanol, C2H5OH(L) resulted in a rise in temperature from 16.5 °C to 20.9 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184...
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