Acetylene ( C 2 H 2 ) is hydrogenated to form ethane ( C 2 H 6 ) The feed to the reactor contains 1 5 0 mol H 2 m o l C 2 H 2 a Calculate the stoichiometric reactant ratio ( m o l H 2 react m o l C 2 H 2 react ) and the yield ratio ( k m o l C 2 H 6 formed k m o l H 2 react ) b Determine the limiting reactant and calculate the percentage by which the other reactant is in excess c Calculate the mass feed rate of hydrogen ( k g s ) required to produce 4 1 0 6 tons of ethane per year assuming that the reaction goes to completion and that the process operates for 2 4 hours a day, 3 0 0 days a year Ethane ( C 2 H 6 ) is chlorinated in a continuous reactor C 2 H 6 C l 2 C 2 H 5 C l H C l Some of the product monochloroethane ( C 2 H 5 C l ) is further chlorinated in an undesired side reaction to produce dichloroethane ( C 2 H 4 C l 2 ) C 2 H 5 C l C l 2 C 2 H 4 C l 2 H C l a Take a basis of 1 0 0 m o l C 2 H 5 C l produced Assume that the feed contains only ethane and chlorine, and that all chlorine is consumed Draw and label the flow chart and carry out a degree of freedom analysis twice ( once using atomic atomic balance method and once using extent of reaction method ) b The reactor is designed to achieve a 1 5 conversion of ethane and a selectivity of 1 4 mol C 2 H 5 C l m o l C 2 H 4 C l 2 , with a negligible amount of chlorine in the product gas Calculate i All unknown variables ( flow rates ) ii The feed ratio ( molC l 2 m o l C 2 H 6 ) iii The fractional yield of monochloroethane 3 Butane is burned with air No carbon monoxide is present in the combustion products a Use the degree of freedom analysis to prove that if the percentage excess air and the percentage conversion of butane are specified, the molar composition of the product gas can be determined b Calculate the molar composition of the product gas for each of the following three cases i Theoretical air supplied and 1 0 0 conversion of butane ii 2 0 excess air and 1 0 0 conversion of butane iii 2 0 excess air, 9 0 conversion of butane Solve all qustions

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Acetylene ( C 2 H 2 ) is hydrogenated to form ethane ( C 2 H 6 ) . The feed to the reactor contains

Acetylene

(C_{2} H_{2})

is hydrogenated to form ethane

(C_{2} H_{6}) .

The feed to the reactor contains

1.50

mol

\frac{H_{2}}{m} o l C_{2} H_{2} .

.

Calculate the stoichiometric reactant ratio

(m o l H_{2}

react

\frac{?}{m o l C_{2} H_{2}}

react

)

and the yield ratio

(k m o l C_{2} H_{6}

formed

\frac{?}{k m o l H_{2}}

react

) .

.

Determine the limiting reactant and calculate the percentage by which the other reactant is in excess.

.

Calculate the mass feed rate of hydrogen

(k \frac{g}{s})

required to produce

4 10^{6}

tons of ethane per year assuming that the reaction goes to completion and that the process operates for

24

hours a day,

300

days a year.

Ethane

(C_{2} H_{6})

is chlorinated in a continuous reactor:

C_{2} H_{6} + C l_{2} C_{2} H_{5} C l + H C l

Some of the product monochloroethane

(C_{2} H_{5} C l)

is further chlorinated in an undesired side reaction to produce dichloroethane

(C_{2} H_{4} C l_{2})

C_{2} H_{5} C l + C l_{2} C_{2} H_{4} C l_{2} + H C l

.

Take a basis of

100 m o l C_{2} H_{5} C l

produced. Assume that the feed contains only ethane and chlorine, and that all chlorine is consumed. Draw and label the flow chart and carry out a degree

-

-

freedom analysis twice

(

once using atomic atomic balance method and once using extent of reaction method

) .

.

The reactor is designed to achieve a

15 %

conversion of ethane and a selectivity of

14

mol

C_{2} H_{5} C \frac{l}{m} o l C_{2} H_{4} C l_{2},

with a negligible amount of chlorine in the product gas. Calculate:

.

All unknown variables

(

flow rates

)

.

The feed ratio

(

molC

\frac{l_{2}}{m} o l C_{2} H_{6})

iii. The fractional yield of monochloroethane.

3 .

Butane is burned with air. No carbon monoxide is present in the combustion products.

.

Use the degree

-

-

freedom analysis to prove that if the percentage excess air and the percentage conversion of butane are specified, the molar composition of the product gas can be determined.