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  • Material Balance Calculations - Week 1

    • Checklist - Week-1
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    • Day-1: Material Balance - Theory - Video Page
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    • Day-1-Material Balance - slides Book
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    • Day2: Review, Atomic Balance - Theory Page
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    • Formaldehyde from Methane - Extent of Reaction, Atomic Balance - Example Page

      2021-37-pc

      Formaldehyde is produced by the oxidation of methane in a reactor. The following two parallel reactions occur. \[ \begin {align*} \ce {CH4} + \ce {O2} &\rightarrow \ce {HCHO} + \ce {H2O} \\
      \ce {CH4} + \ce {2O2} &\rightarrow \ce {CO2} + \ce {2H2O} \end {align*} \]       Methane and oxygen are fed to the reactor. The product gases leaving the reactor include methane, oxygen, formaldehyde, carbon dioxide and water vapor.

      60 mol/s of methane enters the reactor. The molar flow rate (in mol/s) of \(\ce {CH4}\), \(\ce {O2}\) and \(\ce {CO2}\) leaving the reactor are 26, 2 and 4, respectively. The molar flowrate of oxygen entering the reactor is ________ mol/s.

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    • Combustion of Propane: Atomic Balance - Extent of Reaction - Workout Page
      1990-11-i-pc

      Pure propane (\(\ce {C3H8}\)) is burnt with an excess of air to give the following analysis of combustion products in volume percent:

      \(\ce {CO2}\) = 5.0, \(\ce {CO}\) = 3.5, \(\ce {H2O}\) = 11.4, \(\ce {O2}\) = 7.0 and \(\ce {N2}\) = 73.1
      Calculate the percentage of excess air used.

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    • Combustion of Methane - Atomic Balance - Extent of Reaction Page

      2010-33-pc

      The products of combustion of methane in atmospheric air (21% O2 and 79% N2) have the following composition on a dry basis:

      Products     Mole %
      CO2 10.00
      O2 2.37
      CO 0.53
      N2 87.10
      The ratio of the moles of CH4 to the moles of O2 in the feed stream is ______

      1. 1.05

      2. 0.60

      3. 0.51

      4. 0.45

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    • Yield, Selectivity of Reactions Page
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    • Yield and Selectivity - Dehydrogenation of Ethane Page
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    • Yield and Selectivity - Ethylene Hydration Reaction Page
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    • Theoretical and Excess Air - Example Page
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    • Combustion of Coal Page
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    • Combustion of Methanol Page
      Felder3E-4-71

      Liquid methanol (density = 792 g/L) is fed to a space heater at a rate of 12 L/h and burned with excess air. The product gas is analyzed and the following dry-basis mole percentages are determined: \(\ce{CH3OH}\) = 0.45%, \(\ce{CO2}\) = 9.03%, and \(\ce{CO}\) = 1.81%.

      1. Calculate the percentage conversion of methanol ______ , the percentage excess air fed ______ , and, mole% of water in the product gas _______.
      2. Calculate the molar flow rate of dry product gas (i.e., excluding water vapor) ______ mol/h, and that of water vapor ________mol/h.
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    • Ethylene Bromide from Ethylene Page
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    • Air Requirement of Claus Plant Page
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  • Material Balance Calculations - Week 2

    • Checklist - Week-2
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    • Weight Loss due to Breathing Page
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    • Blending of Two Liquid Streams Page
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    • Combustion of Pentane Page
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    • Chlrorination of Benzene Page
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    • Preparation of Mixed Acid Page
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    • Evaporation of Spent Lye Page
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    • Mixed Fertilizer Formulation Page
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    • Removal of Water by Bubbling Air Page
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    • Removal of Hexane from Gas by Condensation Page
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    • Drying of CaCO3 Slurry Page
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    • Ethanol from Ethylene - Recycle, Purge Page
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    • HW: Combustion Page
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    • Condensation of Moisture in Air-Conditioning Process Page
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    • Loss of Octane due to Vaporization Page
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  • Energy Balance Calculations

    • Checklist
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    • Theory with Examples Page
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    • Condensation of Moisture from Air Page
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    • Steam Mixing Page
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    • Heat Released from Reaction Page
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    • Adiabatic Flame Temperature of Natural Gas Combustion Page
      Felder3E-9-63
      A natural gas containing 82 mole% \(\ce{CH4}\) and the balance \(\ce{C2H6}\) is burned with 20% excess air in a boiler furnace. The fuel gas enters the furnace at 298 K, and the air is preheated to 423 K. The heat capacities of the stack gas components may be assumed to have the following constant values:

      Component \(C_P\) [(J/(mol.K)]

      \(\ce{CO2}\)

      50.0

      \(\ce{H2O(g)}\)

      38.5

      \(\ce{O2}\)

      33.1

      \(\ce{N2}\)

      31.3

      Standard heat of formation values are as follows:

      Component \(\Delta H_f^\circ\) (kJ/mol)

      \(\ce{CH4}\)

      \(-74.85\)

      \(\ce{C2H6}\)

      \(-84.67\)

      \(\ce{CO2}\)

      \(-393.50\)

      \(\ce{H2O(g)}\)

      \(-241.83\)
      1. Assuming complete combustion of the fuel, calculate the adiabatic flame temperature.
      2. How would the flame temperature change if the percent excess air were increased?
      3. How would the flame temperature change if the percent methane in the fuel were increased?
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    • Maximum Allowable Conversion of Exothermic Reaction Page

      2002-13-pc

      Ammonia is produced by the following reaction \[ \text{N}_2 + 3\text{H}_2 \rightleftharpoons 2\text{NH}_3 \] In a commercial process for ammonia production, the feed to an adiabatic reactor contains 1 kmol/s of nitrogen and stoichiometric amount of hydrogen at 700 K. What is the maximum allowable conversion (in percentage) in the reactor, if the adiabatic temperature rise across the reactor should not exceed 100 K. Assume the feed and product streams to be ideal gas mixtures. The heat of reaction at 700 K for the above reaction is calculated to be -94.2 kJ/mol. Mean molar heat capacities (\(C_P\)), in the range  700 - 800 K, are 0.03, 0.0289 and 0.0492 kJ/mol.K for nitrogen, hydrogen and ammonia respectively.

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    • Heat Loss from the Combustion System Page

      2014-42-pc

      Carbon monoxide (CO) is burnt in presence of 200% excess pure oxygen and the flame temperature achieved is 2298 K. The inlet streams are at 25oC. The standard heat of formation (at 25oC) of CO and CO2 are -110 kJ.mol-1 and -390 kJ.mol-1, respectively. The heat capacities (in J.mol-1.K-1) of the components are \[ C_{P_{\text{O}_2}}= 25 + 14\times10^{-3}T \qquad C_{P_{\text{CO}_2}} = 25 + 42\times10^{-3}T \] where, \(T\) is the temperature in K. The heat loss (in kJ) per mole of CO burnt is _______.

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    • Calorific Value of Fuels Page
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    • Adiabatic Mixing of Steam Page
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    • Heat of Formation from Heat of Combustion Data Page
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    • Heat Transferred from Reactor Page
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    • Adiabatic Combustion of Methane Page
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    • Isothermal Operation of Combustor to Convert Carbon and CO2 to CO Page
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      1997-13-pc

      A feed at 1298 K, consisting of flue gas (\(\ce {CO2}\), \(\ce {O2}\) and \(\ce {N2}\)) and air, is passed through a bed of pure carbon. The reactions that occur both go to completion. \[ \begin {align*} \ce {CO2(g)} + \ce {C(s)} &\rightarrow 2\ce {CO(g)}, \quad \Delta H^\circ _R \text { at 298 K = 170 kJ/mol} \\
      \ce {O2(g)} + 2\ce {C(s)} &\rightarrow 2\ce {CO(g)}, \quad \Delta H^\circ _R \text { at 298 K = \(-\)220.4 kJ/mol} \end {align*} \]       The combustor is adiabatic and the product gases exit at 1298 K. Calculate the required moles of \(\ce {CO2}\) per mole of \(\ce {O2}\) in the feed stream, so that the net heat generated is zero and the bed temperature remains constant at 1298 K.
      Data: Mean molar heat capacities, \(C_{Pm}\)

      Substance \(\ce{C}\) \(\ce{O2}\) \(\ce{CO}\) \(\ce{CO2}\)
      \(C_{Pm}\) (kJ/mol.K) 0.02 0.03 0.03 0.05
    • Heat Released from Combustion of CO Page
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  • Review-1

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    • Molecular Formula from Composition Data Page
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    • Mass Fraction to Mole Fraction Page
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    • Volume of Gas Required for a Given Composition Page
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    • Degree of Freedom Analysis for a Splitter Page
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    • Degree of Freedom Analysis for Combustion System Page
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    • Unsteady Mass Balance - Salt Dissolution Page
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    • Concentration of Solutions Page
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    • Conversion of Gaseous Reaction - Extent of Reaction and Volume Expansivity Factor Approaches Page
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    • Volume of Gas Collected from Reaction of CaCO3 with HCl Page
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    • Coal Sample Analysis Page
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    • Crystallization of Na2SO4 Page
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    • Recovery of Oil by Extraction Page
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    • Capacity of Evaporator Page
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    • Conversion of SO2 in Secondary Converter Page
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  • Review-2

    • Composition of Feed for the Given Excess Air Page
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    • Excess Air from Flue Gas Data Page
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    • Composition of Product from the given Conversion Page
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    • Recycle Rate for the given Conversion Page
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    • Limiting Reactant and Percent Excess Page
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    • Drying of Solid Page
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    • Evaporation - Mass Balance Page
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    • Solubility of Salt Page
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    • Excess Air and Adiabatic Flame Temperature Page
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    • Heat of Reaction from Heat of Combustion Page
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  • Review-3

    • Moles of a Compound for a Mass Fraction Page
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    • Molarity of Sulphuric Acid Solution Page
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    • CaO from Limestone Page
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    • K2O Equivalent of KCl Page
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    • Chlorine from NaCl Brine Page
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    • Preparation of Saturated MnSO4 Solution Page
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    • H/C of Fuel from Orsat Analysis Page
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    • Energy Balance for Production of Acetylene Page
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    • Temperature vs Time Curve for Heating of Water Page
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  • Assessments