i need help with all parts in this question asap Methane (CH₄) reacts with oxygen gas (O₂) to produce formaldehyde (HCHO) in the presence of a catalyst. Unfortunately, methane can also oxidize into carbon dioxide (CO₂) and water vapor (H₂O):\[ \text{CH}_4 + \text{O}_2 \rightarrow \text{HCHO} + \text{H}_2\text{O} \]\[ \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \]The feed to the reactor contains equimolar amounts of methane and oxygen gas. Use a feed stream of 100 mol/s as a basis. The fractional conversion of methane is 0.9 and the fractional yield of formaldehyde is 0.855.(a) Plot a diagram illustrating the process.(b) What are the two extents of reaction, ξ₁ and ξ₂?(c) Determine the molar fraction of each component in the product stream.

Given: 100 mol/s of feed, contains equimolar of methane and oxygen i.e. 50 moles of methane and 50 moles of oxygen Fractional conversion of methane is 0.9 Fractional yield of formaldehyde is 0.855 CH4+O2→HCHO+H2OCH4+2O2→CO2+2H2O a) Process diagram: Methane and oxygen reacts in reactor: Desired product is formaldehyde, undesired product is CO2 and waterb) From given: Fractional conversion of methane is 0.9 Fractional yield of formaldehyde is 0.855 Fractional conversion=Moles reactedMoles fed0.9=Moles reacted50Moles reacted of methane=45 Fractional yield=HCHO in exitCH4 in feed0.855=HCHO in exit50HCHO in exit=42.75 Extent of reaction: CH4+O2→HCHO+H2O...1)CH4+2O2→CO2+2H2O...2) For reaction 1) nCH4=50-ξnO2=50-ξnHCHO=ξnH2O=ξ Unreacted methane: =(1-0.9)×50=5 mol/s nCH4=50-ξ5=50-ξξ=45 nO2=50-45=5nHCHO=45nH2O=45 Answer: Extent of reaction is 45For reaction 2) Unreacted CH4: =(1-0.9)×5=0.5 nCH4=5-ξ0.5=5-ξξ=4.5nO2=50-2ξnO2=41nCO2=4.5nH2O=9 Answer: Extent of reaction is 4.5c) Mole fraction of product component in product stream: From reaction 1) Component Moles Mole fraction HCHO 45 0.5 H2O 45 0.5 Total 90 1 From reaction 2) Component Moles Mole fraction CO2 4.5 0.337 H2O 9 0.667 Total 13.5 1