Question

In: Other

Consider a 100 mol mixture that is 69.0% methane (CH4) and 31.0% ethane (C2H6). To this...

Consider a 100 mol mixture that is 69.0% methane (CH4) and 31.0% ethane (C2H6). To this mixture is added 20.0% excess air. Of the methane present, 90.40% reacts, 92.30% of which forms carbon dioxide (CO2), and the balance forms carbon monoxide (CO). Of the ethane present, 86.0% reacts, 92.30% of which forms carbon dioxide, and the balance forms carbon monoxide.

a) What is the theoretical amount of oxygen required for the fuel mixture?

b) What amount of air is added to the fuel mixture?

c) How many moles of methane are present in the product gas?

d) How many moles of ethane are present in the product gas?

e) How many moles of carbon dioxide are present in the product gas?

f) How many moles of carbon monoxide are present in the product gas?

g) How many moles of water vapor are present in the product gas?

h) How many moles of oxygen are present in the product gas?

i) How many moles of nitrogen are present in the product gas?

Solutions

Expert Solution

Methane combustion reactions

CH4 + 2O2 = CO2 + 2H2O

CH4 + 1.5O2 = CO + 2H2O

ethane combustion reactions

C2H6 + 3.5O2 = 2CO2 + 3H2O

C2H6 + 2.5O2 = 2CO + 3H2O

At inlet

Moles of CH4 = 100 x 0.69 = 69 mol

Moles of C2H6 = 100 x 0.31 = 31 mol

CH4 reacted = 0.904 x 69 = 62.376 mol

CO2 produced from CH4 = 0.923 x 62.376 = 57.573 mol

CO produced from CH4 = (1 - 0.923) x 62.376 = 4.803 mol

C2H6 reacted = 0.86 x 31 = 26.66 mol

CO2 produced from C2H6 = 0.923 x 26.66 x 2 = 49.22 mol

CO produced from C2H6 = (1 - 0.923) x 26.66 x 2 = 4.10 mol

Part a

O2 required for CH4 combustion = 3.5 x 69 = 241.5 mol

O2 required for C2H6 combustion = 6 x 31 = 186 mol

theoretical amount of oxygen required for the fuel mixture

= 241.5 + 186 = 427.5 mol

Part b

Air fed = 1.2 x 427.5 = 513 mol

Air added = 513 - 427.5 = 85.5 mol

Part c

moles of methane are present in the product gas

= moles of CH4 at inlet - moles of CH4 reacted

= 69 - 62.376

= 6.624 mol

Part d

moles of ethane are present in the product gas

= moles of C2H6 at inlet - moles of C2H6 reacted

= 31 - 26.66

= 4.34 mol

Part e

moles of carbon dioxide are present in the product gas

= CO2 produced from CH4 + CO2 produced from C2H6

= 57.573 + 49.22

= 106.793 mol

Part F

moles of carbon dioxide are present in the product gas

= CO produced from CH4 + CO produced from C2H6

= 4.803 + 4.10

= 8.903 mol


Related Solutions

A mixture of methane (CH4) and ethane (C2H6) is stored in a container at 294 mm...
A mixture of methane (CH4) and ethane (C2H6) is stored in a container at 294 mm Hg. The gases are burned in air to form CO2 and H2O. If the pressure of CO2 is 346 mm Hg measured at the same temperature and volume as the original mixture, calculate the mole fraction of the gases. Mole fraction of methane: _____________ Mole fraction of ethane: _________________
A gaseous fuel mixture contains 20.7% methane (CH4), 44.0% ethane (C2H6) and the rest propane (C3H8)...
A gaseous fuel mixture contains 20.7% methane (CH4), 44.0% ethane (C2H6) and the rest propane (C3H8) by volume. Part A When the fuel mixture contained in a 1.57 L tank, stored at 756 mmHg and 298 K, undergoes complete combustion, how much heat is emitted? (Assume that the water produced by the combustion is in the gaseous state.) Express your answer with the appropriate units.
A natural gas has the following composition: CH4 (methane) = 87 %, C2H6 (ethane) = 12...
A natural gas has the following composition: CH4 (methane) = 87 %, C2H6 (ethane) = 12 %, and C3H8 (propane) = 1 %. a.) What is the composition in weight percent? b.) What is the composition in volume percent? c.) How many cubic meters will be occupied by 80.0 kg of the gas at 9 °C and 600 kPa? d.) What is the density of the gas in kilograms per cubic meter at standard conditions? e.) What is the specific...
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount...
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount of propane, C3H8) were added to the same 10.0-L container. At 23.0 ∘C, the total pressure in the container is 5.00 atm . Calculate the partial pressure of each gas in the container. Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane. Part B A gaseous mixture of O2 and N2 contains...
part A)Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown...
part A)Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount of propane, C3H8) were added to the same 10.0-L container. At 23.0 ∘C, the total pressure in the container is 4.80 atm . Calculate the partial pressure of each gas in the container. Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane. Part B) A gaseous mixture of O2 and N2...
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount...
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount of propane, C3H8) were added to the same 10.0-L container. At 23.0 ∘C, the total pressure in the container is 4.60 atm . Calculate the partial pressure of each gas in the container. Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane.
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount...
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount of propane, C3H8) were added to the same 10.0-L container. At 23.0 ∘C, the total pressure in the container is 3.60 atm . Calculate the partial pressure of propane in the container.
A mixture of hydrocarbons (10mol% methane, 20 mol% ethane, 30mol% propane, 15mol% isobutane, 20 mol% n-butane,...
A mixture of hydrocarbons (10mol% methane, 20 mol% ethane, 30mol% propane, 15mol% isobutane, 20 mol% n-butane, 5 mol% n-pentane) is flashed into a separator at 80 F and 150 psia. What fraction leaves the separator as liquid and what is its composition?
A mixture of 0.05263 mol of H2O, 0.01327 mol of CH4, 0.07198 mol of CO, and...
A mixture of 0.05263 mol of H2O, 0.01327 mol of CH4, 0.07198 mol of CO, and 0.06917 mol of H2 is placed in a 1.0-L steel pressure vessel at 1303 K. The following equilibrium is established: 1 H2O(g) + 1 CH4(g) 1 CO(g) + 3 H2(g) At equilibrium 0.009871 mol of CH4 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of H2O, CH4, CO, and H2. Peq(H2O) = . Peq(CH4) = . Peq(CO) = . Peq(H2)...
10. A mixture of 0.08729 mol of H2O, 0.1041 mol of CH4, 0.08069 mol of CO,...
10. A mixture of 0.08729 mol of H2O, 0.1041 mol of CH4, 0.08069 mol of CO, and 0.1098 mol of H2 is placed in a 1.0-L steel pressure vessel at 1034 K. The following equilibrium is established: 1 H2O(g) + 1 CH4(g) 1 CO(g) + 3 H2(g) At equilibrium 0.06283 mol of CO is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of H2O, CH4, CO, and H2. Peq(H2O) = ____ . Peq(CH4) = ____ . Peq(CO)...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT