Uploaded December 2022 | Updated September 2026, 2 weeks ago
Students of the Fall 2022 Semester
Professor DeBacco
Student Introductions
As a teacher it is important to pass on what you have learned and see where your students take that information.
It has been great working with both Kiera and Connor and hopefully you have also enjoyed some of the videos they have appeared in.
This video will help provide a brief introduction to both students…
Kiera
Has shown continued interest in cannabis production beyond the course work.
She has appeared in DeBacco University videos and is continually expanding her education and enjoys sharing this with others.
YouTube: youtube.com/channel/UCxJ2wMI84bN6dI7tFje2ezA
Instagram: instagram.com/kannakiera/?hl=en
Connor
After taking both the Introduction to Cannabis Horticulture and also the Advanced Cannabis Horticulture Connor is now the lead cultivator at a large production greenhouse operation.
The information from the course has proven to be helpful on a daily basis and he has been willing to share some of his experiences here on DeBacco University.
Link to Lecture Slides: drive.google.com/file/d/1LXBDBq0h0AYqSCB48rz1YMItzV1veW2h/view?usp=share_link
*Due to the description character limit the full work cited for "Students of the Fall 2022 Semester" can be viewed at... docs.google.com/document/d/1vZkwdonhiEK84mxF3Hr1fjrefU1qjLVk/edit?usp=share_link&ouid=104237452697237972847&rtpof=true&sd=true
Students of the Fall 2022 Semester
Professor DeBacco
Student Introductions
As a teacher it is important to pass on what you have learned and see where your students take that information.
It has been great working with both Kiera and Connor and hopefully you have also enjoyed some of the videos they have appeared in.
This video will help provide a brief introduction to both students…
Kiera
Has shown continued interest in cannabis production beyond the course work.
She has appeared in DeBacco University videos and is continually expanding her education and enjoys sharing this with others.
YouTube: youtube.com/channel/UCxJ2wMI84bN6dI7tFje2ezA
Instagram: instagram.com/kannakiera/?hl=en
Connor
After taking both the Introduction to Cannabis Horticulture and also the Advanced Cannabis Horticulture Connor is now the lead cultivator at a large production greenhouse operation.
The information from the course has proven to be helpful on a daily basis and he has been willing to share some of his experiences here on DeBacco University.
Link to Lecture Slides: drive.google.com/file/d/1LXBDBq0h0AYqSCB48rz1YMItzV1veW2h/view?usp=share_link
*Due to the description character limit the full work cited for "Students of the Fall 2022 Semester" can be viewed at... docs.google.com/document/d/1vZkwdonhiEK84mxF3Hr1fjrefU1qjLVk/edit?usp=share_link&ouid=104237452697237972847&rtpof=true&sd=true





![Calculating Net Energy Change of a Reaction
Calculating Net Energy Change of a Reaction
Dr. DeBacco
How Its Calculated Using Bond Enthalpies
If you know the bond enthalpies of all bonds broken and formed:
ΔH = Σ (Bond energies of bonds broken) − Σ (Bond energies of bonds formed)
In other words:
Breaking bonds = energy absorbed/input (endothermic)
Forming bonds = energy released/output (exothermic)
Higher bond energy = stronger bond
So the heat of reaction tells you the net energy flow for the whole process.
Net Energy Change
To calculate the net energy change of a chemical reaction, you are essentially figuring out how much energy is absorbed or released when bonds are broken and formed.
Formula for Net Energy Change (ΔH)
ΔH = Σ(Bond energies of bonds broken) − Σ(Bond energies of bonds formed)
Breaking bonds → requires energy (positive values)
Forming bonds → releases energy (negative values)
Step-by-Step Guide
Write the balanced chemical equation.
Make sure all reactants and products are accounted for.
List all bonds broken in the reactants.
Count how many of each type of bond is broken.
List all bonds formed in the products.
Count how many of each type of bond is formed.
Use average bond energies
These are typically found in tables (e.g., C–H ≈ 413 kJ/mol, O=O ≈ 495 kJ/mol).
Plug into the formula.
Add up the energy for all bonds broken and subtract the energy for all bonds formed.
Example: Combustion of Methane
CH₄ + 2O₂ → CO₂ + 2H₂O
Bonds broken:
4 × C–H (413 kJ/mol)
2 × O=O (495 kJ/mol)
Bonds formed:
2 × C=O (799 kJ/mol)
4 × O–H (463 kJ/mol)
ΔH = [4×413 + 2×495] − [2×799 + 4×463] ΔH = [1652 + 990] − [1598 + 1852] ΔH = 2642 − 3450 = −808 kJ/mol
This reaction is exothermic, releasing 808 kJ/mol of energy.
Link to Lecture Slides: https://drive.google.com/file/d/1RVZ77V5Vt6CWEoUCQJ9D9PV3Ds_sefFR/view?usp=drive_link
*Due to the description character limit the full work cited for Calculating Net Energy Change of a Reaction can be viewed at... https://docs.google.com/document/d/1o4ZSu6akSk xD_8q9gyRspC_EypGy-b/edit?usp=drive_link&ouid=104237452697237972847&rtpof=true&sd=true Calculating Net Energy Change of a Reaction](https://i.ytimg.com/vi/iHWwrt6rrWU/mqdefault.jpg)




