3. Methane is burned with air in a continuous steady-state combustion reactor to yield a mixture of carbon monoxide, carbon dioxide, and water. The feed to the reactor contains \( 12 \mathrm{~mole}_{\mathrm{o}} \mathrm{CH}_{4}, 25 \% \) \( \mathrm{O}_{2} \), and \( 63 \% \mathrm{~N}_{2} \). The percentage conversion of methane is \( 80.0 \% \), and the gas leaving the reactor contains \( 4 \mathrm{~mol} \mathrm{CO} 2 / \mathrm{mol} \mathrm{CO} \). Please write down the reactions, draw the flowchart and write everything on it. Carry out a degree-of-freedom analysis on the process. Then calculate the molar composition of the product stream. (20 points)
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13.48 Methane $\left(\mathrm{CH}_{4}\right)$ at $25^{\circ} \mathrm{C}, 1$ atm, enters an insulated reactor operating at steady state and burns with the theoretical amount of air entering at $25^{\circ} \mathrm{C}, 1 \mathrm{~atm}$. The products contain $\mathrm{CO}_{2}, \mathrm{CO}, \mathrm{H}_{2} \mathrm{O}, \mathrm{O}_{2}$, and $\mathrm{N}_{2}$, and exit at $2260 \mathrm{~K}$. Determine the fractions of the entering carbon in the fuel that burn to $\mathrm{CO}_{2}$. and $\mathrm{CO}$, respectively.
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Methane is burned to form carbon dioxide and water in a batch reactor: CH4 + 2O2 → CO2 + 2H2O The feed to the reactor and the products obtained are shown in the following flowchart: 100 mol CH4 250 mol O2 40 mol CH4 130 mol O2 60 mol CO2 120 mol H2O 1. How much methane was consumed? What is the fractional conversion of methane? 2. How much oxygen was consumed? What is the fractional conversion of oxygen? 3. Write the extent of reaction equation (4.6-4) for methane, oxygen, and CO2. Use each equation to determine the extent of reaction, ́̑, substituting inlet and outlet values from the flowchart. 4. How many independent molecular species balances can be written? How many independent atomic species balances can be written? 5. Write the following balances and verify that they are all satisfied. The solution of the first one is given as an example. (a) Methane. (I = O + C ⟹ 100 mol CH4 in = 40 mol CH4 out + 60 mol CH4 consumed) (b) Atomic oxygen (O). (c) Molecular oxygen (O2). (d) Water. (e) Atomic hydrogen.
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Methane (CH4) is burned with atmospheric air. The analysis of the products on a dry basis is as follows: CO2 = 10%, O2 = 2.37%, CO = 0.53%, N2 = 87.10%. (i) Determine the combustion equation; (ii) Calculate the air-fuel ratio; (iii) Percent theoretical air.
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