1. Not finding help here? Sign up for a free 30min tutor trial with Chegg Tutors
    Dismiss Notice
Dismiss Notice
Join Physics Forums Today!
The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

Heat Recovery from Boiler Exhaust Gases

  1. Jan 2, 2015 #1
    1. The problem statement, all variables and given/known data
    The exhaust gases from a natural gas-fired central heating boiler leave the boiler at a temperature of 70 deg C. The oxygen content of the exhaust gases is 9% by volume (dry). The rate of energy input (Gross calorific value) to the boiler from natural gas is 16kW. The gross calorific value of natural gas is 55MJ/kg. For the purposes of all calculations assume that natural gas is 100% Methane (CH4). The pressure in the combustion chamber of the boiler and throughout the heat recovery system is 1 bar.

    The exhaust gases are blown down a plastic pipe situated in a room are then exhausted to atmosphere, as shown in the diagram attached. The warm pipe provides a heat input to the room of 0.75kW. The pipe is 100mm in diameter and is made up of a number sections 1m in length.

    The overall heat transfer coefficient (U) for heat transfer from the exhaust gases through the pipe to the room is 9.5 W/m^2K. The room temperature is 20 deg C.

    Calculate:
    1. The temperature to which the exhaust gases must be cooled in order to recover 0.75kW of heat.
    2. The number of 1m length of pipe needed to provide the heat input of 0.75kW to the room.

    2. Relevant equations
    Hints:
    The best way to calculate the final temperature of the exhaust gases is to consider cooling down to a different temperatures and identifying (by iterating between the nearest values) which temperature gives 0.75kW of heat recovery.

    To calculate the heat recovery from the exhaust gases as they cool through a temperature difference of Delta T, use Q = mCpDeltaT for the dry products of combustion and Q = mDeltah for the water vapour, where appropriate enthalpy values are taken from tables. (A temperature interval of about 5 deg C is appropriate).

    As the exhaust gas temperature varies along the pipe, the best way to calculate the length needed is to consider each temperature interval, assume a mean gas temperature, then calculate the length of the pipe needed to give the heat transfer between the exhaust gas and the room as the gas cools over the temperature interval.

    3. The attempt at a solution

    CH4 + x 02 + 3.76x N2 = a CO2 + b H20 + c 02 + d N2

    a = 1
    b = 2
    x = 2 + c
    d = 3.76x = 3.76(2 + c) = 7.52 + 3.76c

    9% oxygen, dry
    0.09 = c / (a+c+d)
    0.09 = c/(1+c+7.52 + 3.76c)
    c = 1.3417 moles

    and thus x = 3.417 moles

    Reactant
    mass (Molar Mass * moles)
    CH4 1 moles 16 * 1 = 16kg

    Products
    mass (Molar Mass * moles) mass/kg fuel
    CO2 1 mole 44*1 = 44kg 44/16 = 2.75kg/kg fuel
    H2O 2 moles 18*2 = 36 kg 36/16 = 2.25kg/kg fuel
    O2 1.3417 moles 32*2 = 42.9344kg 42.934/16 = 2.6834kg/kg fuel
    N2 12.565 moles 28*12.565 = 351.82 kg 351.82/16 = 22kg/kg fuel

    I am completely clueless on how to continue afterwards. The hint told me to make an assumptions of the final temperature that will allow a heat recovery of 0.75 kW.

    By using the formula:

    Q = ∑(mass of dry product*Cp* ΔT) + mass of H2O * enthalpy of steam at 70 deg C - (mass of H20 water * enthalpy of water at assumed Temp + mass of H2O vapour * enthalpy of steam at assumed temperature)

    I found the mass of water= 0.0985kg and the water vapour= 0.110864kg.
    I work on excel spread sheet, taking the assumptions of the temperature from 0 deg to 35 deg, all give me the answer of more than 0.75 kW, the required output. At 1.5 deg, the heat recovery is found to be 7510kW, an outrageous amount compared to the required 0.75kW. Could you please help?

    Thank you in advance.
     

    Attached Files:

  2. jcsd
  3. Jan 2, 2015 #2

    BvU

    User Avatar
    Science Advisor
    Homework Helper
    Gold Member

    How many kg/s of CH4 do you feed the boiler ? How many kg/s of exhaust gas does that yield ?

    Then: if the room temperature is 20 degrees, what is the minimum exhaust temperature to the outside world ?

    The exercise instruction to consider the water in the exhaust from the boiler to be in the vapour phase at 70 degrees and 1 Bar is clear, but not very realistic, I would say.
     
    Last edited: Jan 2, 2015
  4. Jan 2, 2015 #3
    As BvU indicated, you need to start out by determining the mass flow rate through the exhaust pipe. You are given the heat transfer rate from the exhaust pipe to the room(0.75 kW). From this, you can calculate the exit temperature from the exhaust pipe. Don't forget to take into account the heat of condensation for the part of the water vapor that condenses (probably most of it by the exit). Once you know the exit temperature, you need to calculate the part of the heat load occurring over 5C increments within the pipe. From this, you can use the overall heat transfer coefficient and the room air temperature to determine the length of each section required to bring about each 5 C increment. You then add these up to get the overall length.

    Chet
     
  5. Jan 2, 2015 #4
    Why do you think this? What is the partial pressure of the water vapor in the exhaust? What is the equilibrium vapor pressure of water at 70C?

    Chet
     
  6. Jan 2, 2015 #5

    BvU

    User Avatar
    Science Advisor
    Homework Helper
    Gold Member

    Thanks for putting me right, Chet. Oh boy, what a beginner's mistake. Please disregard altogether, nightingale.

    But do ask yourself how many kg/s of CH4 the boiler needs to generate 16 kW.
     
  7. Jan 2, 2015 #6
    This is not as straightforward a calculation as it seems. Nightingale has to do an overall open system first law heat balance on the boiler, and has to take into account the enthalpy of the exhaust stream exiting the boiler (which will be significant). Also, the 55 MJ/kg is the heat of combustion at 25 C, assuming liquid water is part of the product stream. Nightingale also has to make some kind of assumption regarding the temperature of the feed air and methane to the boiler (20 C for each is reasonable).

    It will be interesting to see how nightingale does this calculation.

    Chet
     
  8. Jan 2, 2015 #7

    BvU

    User Avatar
    Science Advisor
    Homework Helper
    Gold Member

    Time for a tweet from Nightingale, then !
     
  9. Jan 3, 2015 #8
    Thank you Chet and BvU.

    I found that the fraction of water vapour can be calculated from= 2 moles/ 16.91 (total moles in the product) * 100% = 11.827%.
    The pressure of the system is 1 bar, thus partial pressure of water vapour in the flue gases is 0.11827* 1 bar= 0.11827 bar, and from the steam tables, at 0.11827 bar, the water vapour will start to condense at 49.1 deg C.

    Both of you advised me to obtain the mass flow rate:
    I assume the inlet air to be 25°C.
    Q = m (mass flow rate of CH4)* [∑m (mass of dry products) * Cp *(T1 - T2) + mH2O * (hg at 70°C - hf at 25°C)]
    Q = m * [2.75* 0.871 (CO2) +2.6834*0.923 (O2) +22*1.04 (N2)] * (70 - 25) + 2.25 * (2626.3-104.8)
    16 = m *1248*5673.375
    m = 2.26*10^(-6) kg/s


    Am I going in the right way?
    Please bear with me, I took this subject as an extra module and I am struggling to understand. Thank you very much!
     
    Last edited: Jan 3, 2015
  10. Jan 3, 2015 #9

    BvU

    User Avatar
    Science Advisor
    Homework Helper
    Gold Member

    That would be a cheap gas bill :)

    Isn't the Q you calculate this way the heat needed to bring the exhaust products from 25 to 70 degrees ?
    What happened to the 55 MJ/kg ?
    And why does a + sign change to a * suddenly ?
    And is the 16 really 16 ?
     
  11. Jan 3, 2015 #10
    Hi nightingale,

    Nice job on getting the dew point.

    As far as the heat balance on the boiler is concerned, there are a few improvements needed. Since your mass balances were done on the basis of 1 kg-mole of methane, it would be easier to base the heat balance on the molar flow rate of methane to the reactor. So, let m represent the inlet molar flow rate of methane in kg-mole/sec. You can then easily calculate the rate of sensible heat exiting the boiler. In this case, you would directly use the moles of the various species in the exit stream calculated from your mass balance, and you would use molar heat capacities, rather than mass heat capacities. Also, in the case of the water, you would multiply the enthalpies from your steam table by 18. If your mass flow rate m is in kg-moles/sec of methane fed to the reactor, then the sensible heat rate of your exit stream will be kW.

    As BvU indicated, you omitted the heat of combustion from the boiler heat balance. That should be on the right side of the equation, and you have to convert that to kJ/kg-mole (multiply by 16) and you also have to multiply it by the inlet molar flow rate of methane m. The 16 kW is subtracted from this, since it is being transferred from the combustion gases to make the steam.

    Chet
     
  12. Jan 3, 2015 #11
    Yes, thank you for pointing that out.
    Does this mean I have to convert 55MJ/kg into watt and then subtract 16 from it to obtain the Q?
     
  13. Jan 3, 2015 #12
    I'm confused on how do I change the base of my calculations into molar flow rate of methane. It was:
    Q = m (mass flow rate of CH4)* [∑m (mass of dry products/kg fuel of Methane) * Cp *(T1 - T2) + mH2O * (hg at 70°C - hf at 25°C)]
    Q = m * [2.75* 0.871 (CO2) +2.6834*0.923 (O2) +22*1.04 (N2)] * (70 - 25) + 2.25 * (2626.3-104.8)
    16 = m *1248+5673.375
    m = 2.3*10^(-3) kg/s.... which is wrong because I did not take into account the heat of combustion.

    Is it like this then?
    Q = m (molar flow rate of CH4)* [∑m (moles of dry products*Molar of products) * Cp *(T1 - T2) + moles H2O * molarity* (hg at 70°C - hf at 25°C)]
    Q = m * [1*44* 0.871 (CO2) +1.3417*32*0.923 (O2) +12.565*28*1.04 (N2)] * (70 - 25) + 2.25 * 18* (2626.3-104.8)

    But then again by doing that, the result will just be the mass (kg) of the products. I'm really confused, could you please help?

    What is this heat of combustion? Is it a parameter I have to find? Or is it just 16kW * molar flow rate methane * 16? and thus:
    Q = m (molar flow rate of CH4)* [∑m (moles of dry products*Molar of products) * Cp *(T1 - T2) + moles H2O * molarity* (hg at 70°C - hf at 25°C)]+ 16*16*m
    55* 10^3 = m * [1*44* 0.871 (CO2) +1.3417*32*0.923 (O2) +12.565*28*1.04 (N2)] * (70 - 25) + 2.25 * 18* (2626.3-104.8) + 16*16*m

    Thank you
     
  14. Jan 3, 2015 #13
    Your final equation is almost right. It should read:

    55* 10^3(16)m = m * ([1*44* 0.871*44 (CO2) +1.3417*32*0.923 (O2) +12.565*28*1.04 (N2)] * (70 - 25) + 2.25 * 18* (2626.3-104.8)) + 16*10^3

    The corrections are indicated in bold. Note the parenthesis include the water term.

    Chet
     
  15. Jan 4, 2015 #14
    I don't understand why do I have to multiply the molar mass of CO2 twice and why is the 16kW multiplied by 10^3? I thought that since all the heat capacities and masses are in kg, then the unit should be kW, which makes it like this:

    55* 10^3(16)m = m * ([1*44* 0.871 (CO2) +1.3417*32*0.923 (O2) +12.565*28*1.04 (N2)] * (70 - 25) + 2.25 * 18* (2626.3-104.8)) + 16

    Could you please elaborate further? Thank you
     
  16. Jan 4, 2015 #15
    Oops. I missed the 44 in the equation you wrote. Of course, you are right. It should only be there once. Also, somehow I though that the 16 kW was 16 MW.

    Chet
     
  17. Jan 5, 2015 #16
    Thank you Chet,
    I was able to find the mass flow rate with your help and obtain 3.33 * 10^(-4) kg/s. I checked with the teacher, who confirmed the flow rate value. I try to find the answer for the 2nd part:
    2. The temperature to which the exhaust gases must be cooled in order to recover 0.75kW of heat:

    I first assume that the temperature is cooled to around 5 degC and thus took the the Cp, hf and hg based on this. I will recalculate a more precise one later. My first iteration:
    Q = m (mass flow rate of CH4)* [∑m (mass of dry products/kg fuel of Methane) * Cp *(T1 - T2) + mH2O * hg at 70°C -(mass of H2O water *hf + mass of vapour *hg)]
    0.75kW = 0.000333 *(27.752 (70- Temperature of exhaust) + 5923.35 - 277.85)
    2252 = 27.752 (70 - T) + 5645.5
    -3393 = 27.752 (70 - T)
    -122.3 = 70 - T
    T = 192 deg C

    Instead of being cooled, it is being heated! I'm really confused and my teacher couldn't help me at all. Could you please help? Thank you in advance.
     
  18. Jan 5, 2015 #17

    BvU

    User Avatar
    Science Advisor
    Homework Helper
    Gold Member

    Check your math. Brackets have a purpose. It might help if you consistently hang on to units as well.
     
  19. Jan 5, 2015 #18
    Please disregard my answer above. I realized my mistake, where the moles of water and water vapour varies greatly with the temperature and thus my answer will not be valid.
     
  20. Jan 5, 2015 #19

    BvU

    User Avatar
    Science Advisor
    Homework Helper
    Gold Member

    Yes, it will depend on the temperature. With your spreadsheet you can solve that by iterating by hand (or by using the solver).
    And do keep track of what is what (dimensions) and of the brackets (m H2O/kg CH4 , not just m H2O)
     
  21. Jan 5, 2015 #20
    Thank you very much Chet and BvU, I was finally able to find the temperature that will give me 0.75kW heat recovery! Which I found was around 43 degC from the excel spreadsheet (attached if you would like to see).

    My last question:
    How do I find the number of 1m lengths of pipe to provide the heat input of 0.75kW to the room? I don't know where to start, any hints please?
     

    Attached Files:

Know someone interested in this topic? Share this thread via Reddit, Google+, Twitter, or Facebook

Have something to add?
Draft saved Draft deleted



Similar Discussions: Heat Recovery from Boiler Exhaust Gases
Loading...