A gas mixture at 300 degree C and 1 atm is fed to a reactor at 4.7 m^3/hr. The g

Question

A gas mixture at 300 degree C and 1 atm is fed to a reactor at 4.7 m^3/hr. The gas contains 900% by volume ethanol (CH_3CH_2OH) and the balance acetaldehyde (CH_3CHO). The ethanol is dehydrogenated in the reactor to form acetaldehyde and hydrogen gas following the reaction, C_2H_5OH(g) rightarrow CH_3CHO(g)+H_2(g) with the standard heat of reaction (Delta H^0_r at 25 degree C and 1 atm) being 68.95 kJ/mole. To achieve an acceptable conversion rate, external heat is transferred to the reactor at 2583 kJ/hr and the product gas is at 253 degree C and 1 atm. The heat capacities are 0.11. 0.080 and 0.029 kJ/mol degree C for C_2H_5OH, CH_3CHO and H_2, respectively. You are asked to calculate the fractional conversion under the reaction conditions and volumetric flow rate of the product at STP.

Explanation / Answer

Hr,300=Hr,25+viCpT=68.95+(0.029+0.080-0.11)(300-25)=68.675 kJ/mole

Now Q=2583 kJ/hr given

The energy balance for the reaction

Q=niCp,reactant dT+Hr,300

where =fractional conversion

Now reactant F=4.7 m3/hr

ethanol=0.90

acetaldehyde=0.1

So

2583 kJ/hr=4.7 m3/hr(0.9*0.11+0.1*0.08)*(253-300)+68.675*

=37.95 moles/hr

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