Ethanol can be produced commercially by the hydration of ethylene: C2H4 + H2O -> C2H5OH Some...

Ethanol can be produced commercially by the hydration of ethylene:

C2H4 + H2O -> C2H5OH

Some of the product is converted to diethyl ether in the side reaction:

2C2H5OH -> (C2H5)2O + H2O

The feed to the reactor contains ethylene, steam, and an inert gas. A sample of the reactor effluent gas is analyzed and found to contain 43.3 mol% ethylene, 2.5 mol% ethanol, 0.14 mol% ether, 9.3 mol% inerts, and the balance water.

a. Take as a basis 100 mol of effluent gas, draw and label a flowchart, and do a degree of freedom analysis based on an atomic species balance.

b. Calculate the molar composition of the reactor feed, the percentage conversion of ethylene, the fractional yield of ethanol, and the selectivity of ethanol relative to ether.

Expert Solution

Amanda K answered 2 years ago

Ethanol (EtOH) can be produced by the hydration of ethylene, C2H4 + H2O ? C2H5OH, at...

Ethanol (EtOH) can be produced by the hydration of ethylene, C2H4 + H2O ? C2H5OH, at 300?C and high pressure with a phosphoric acid catalyst. Downstream of the reactor, a condenser is used to separate the product, which contains only EtOH and H2O, from a recycle stream that mixes with the fresh feed before entering the reactor. The fresh feed contains 30 mol% C2H4 and the remainder is steam. The single pass conversion is 20%. a. Draw and label the...

Ethanol can be synthesized by direct hydration of ethylene: C2H4(g) + H2O(g) ----> C2H5OH(g). at t...

Ethanol can be synthesized by direct hydration of ethylene: C2H4(g) + H2O(g) ----> C2H5OH(g). at t = 300degC and P = 60 atm. Calculate the yield of the rxn for conditions as above and the equimolar (1:1) input mixture. Use following data: DfH298 (KJ mol-1): C2H4 = 52.4; H20 = -241.8; C2H5OH = -234.8. DfG298 (Kj mol-1): C2H4 = 68.4; H20 = -228.6; C2H5OH = -167.9

Ethylene oxide (C2H4O) is produced by the catalytic oxidation of ethylene (C2H4). That is ethylene is...

Ethylene oxide (C2H4O) is produced by the catalytic oxidation of ethylene (C2H4). That is ethylene is reacted with O2. An undesired side reaction is the combustion of ethylene to CO2 and H2O. The fresh feed to the process consists of oxygen and ethylene. The fresh feed is mixed with a recycle stream, also containing oxygen and ethylene, and fed to the reactor. The feed to the reactor contains a 3:1 molar ratio of ethylene to oxygen. The single pass conversion...

For the reaction described by the chemical equation: C2H4(g) + H2O(l) which yields C2H5OH(l) with a...

For the reaction described by the chemical equation: C2H4(g) + H2O(l) which yields C2H5OH(l) with a delta Hof the reaction=-42.2kJ a) Use the necessary data to calculate the value of delta S of the reaction at 25.0C b)Calculate delta G of the reaction c)In which direction is the reaction, as written, spontaneous at 25C and standard pressure? Forward, reverse, both, neither?

Under which set of conditions will the reaction C2H4(g) + H2O(g) → C2H5OH(g) be nonspontaneous? (ΔG...

Under which set of conditions will the reaction C2H4(g) + H2O(g) → C2H5OH(g) be nonspontaneous? (ΔG is −8.1 kJ.) 10.0 atm C2H4(g), 10.0 atm H2O, and 1.00 atm C2H5OH at 373 K 1.00 atm C2H4(g), 1.00 atm H2O, and 10.0 atm C2H5OH at 373 K 1.00 atm C2H4(g), 1.00 atm H2O, and 1.00 atm C2H5OH at 298 K 1.00 atm C2H4(g),1.00 atm H2O, and 10.0 atm C2H5OH at 523 K

Ethylene oxide is produced by the catalytic oxidation of ethylene: C2H4(g)+12 O2(g)→C2H4O(g) An undesired competing reaction...

Ethylene oxide is produced by the catalytic oxidation of ethylene: C2H4(g)+12 O2(g)→C2H4O(g) An undesired competing reaction is the combustion of ethylene to CO2. The feed to a reactor contains 2 mol C2H4/mol O2. The conversion and yield in the reactor are respectively 25% and 0.70 mol C2H4O produced/mol C2H4 consumed. A multiple-unit process separates the reactor outlet stream components: C2H4and O2 are recycled to the reactor, C2H4O is sold, and CO2 and H2O are discarded. The reactor inlet and outlet...

#1. In the reaction: C2H4(g) + H2O(g) <---> C2H5OH(g) DeltaH = -47.8 kJ Kc = 9.00*103...

#1. In the reaction: C2H4(g) + H2O(g) <---> C2H5OH(g) DeltaH = -47.8 kJ Kc = 9.00*103 @ 600. K a. At equilibrium, PC2H5OH = 200. atm & PH2O = 400. atm. Calculate PC2H4. b. Which set of conditions results in the highest yield of product. Pressure high/low __________ Temperature high/low ________

A.) the standard enthalpy of formation of the reaction C2H4(g)+H2O(l)=C2H5OH(l) B.) Use standard enthalpies of formation...

A.) the standard enthalpy of formation of the reaction C2H4(g)+H2O(l)=C2H5OH(l) B.) Use standard enthalpies of formation to calculate the standard enthalphy change of: the reaction of methane gas, CH4, with chlorine rine to form liquid chloroform, CHCl3. Gaseuous hydrogen chloridee is the other product. C.) Use standard enthalpies of formation to calculate the standard enthalphy change of PCl3(g)+HCl(g)=PCl5(g)+H2(g)

1. Formaldehyde can be produced by oxidation of C2H4 and the following reaction may occur. C2H4...

1. Formaldehyde can be produced by oxidation of C2H4 and the following reaction may occur. C2H4 + ½ O2  C2H4O C2H4 + 3O2  2CO2 + 2H2O Using molecular balance method. Equimolar quantity of C2H4 and O2 was used and the product gas analysis shows 28.57% C2H4O, 11.43% CO2, 11.43% H2O, 22.86% C2H4 and 25.71 % O2. Calculate the % conversion of C2H4 and % Yield of C2H4O.

A gas mixture A composed of 50% ethylene (C2H4) and 50% nitrogen (N2) can be prepared...

A gas mixture A composed of 50% ethylene (C2H4) and 50% nitrogen (N2) can be prepared by blending gas mixture B (20% ethylene and 80% nitrogen by volume) and C (100% ethylene). If 43.3 L (@98.7 atm and 21.1C) of C is used to make mixture A, how many moles of B are needed? How many moles of A can be obtained? N2: Tc = 126.2 K, pc = 33.9 bar C2H4: Tc = 282.8 K, pc = 51.1 bar...

Question