Possible Microwave Effects on Your Biophotons
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Yes, biophotons seem to be tied in with the homeopathy and water memory nonsense...
Article about 1/2 way down the link:
http://www.csicop.org/si/show/alternative_medicine_and_the_laws_of_physics/0 -
Brilliant.No, this is absolute garbage. The wavelength of light that is needed to damage DNA lies in the higher energy regions of the electromagnetic spectrum, the higher end of the Ultra-violet (10 x 10^-9 m to 400 x 10^-9 m), the X-Ray (0.01 x 10^-9 to 10 x 10^-9 m), or the Gamma (< 0.02 x 10^-9 m).
Microwave light lies in the low energy region of the electromagnetic spectrum, or 1 mm to 1 m.
Furthermore, the photon energy required to break one of the chemical bonds of DNA, if we use the canonical equations relating the wavelength of light to the energy of a photon:
E = hν
where E is the energy (J, Joules which is a unit of energy), h is Plank's Constant (6.626 × 10-34 J s), and ν is the frequency (s^-1) of the wavelength of light. The frequency is also expressed in terms of the wavelength
ν= c/λ
where c is the speed of light (2.9979 x 10^8 m/s) and λ is the wavelength of light (in meters, m).
So, the energy for a photon is
E = hc/λ
Plugging in the values for the speed of light, Plank's constant, and the higher end of the Microwave region, or 1 mm (1 x 10^-3 m), the energy of a photon is
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (1 x 10^-3 m) = 1.986 x 10^-22 J
Similarly, the energy of a photon in the lower and upper regions of the Electromagnetic spectrum are
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (400 x 10^-9 m) = 4.966 x 10^-19 J
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (10 x 10^-9 m) = 1.986 x 10^-17 J.
The bond dissociation energy, or the energy required to break the covalent bonds (the class of bond that exists between all of the atoms in DNA). The most common bonds are carbon-hydrogen (C-H), carbon-carbon (C-C), and carbon-nitrogen (C-N) with bond energies 413, 348, and 308 kJ/mol, respectively ( a mol means 6.022 x 10^23 constituent particles or atoms per mol; a mol is a unit).
So, the energy in the weakest bond (in this case the carbon-nitrogen bond is
E = (308 x 10^3 J/mol)/(6.022 x 10^23 mol^-1) = 5.115 x 10^-19 J
THEREFORE, you need to be in the Ultra-violet region of the electromagnetic spectrum.
Thank you. Please stick around.
:glasses: 0 -
Biophotons, beam me up, Scotty0
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sounds legit0
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My biophotons are doing just fine0
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It seems it's another tool in the non-ionizing radiation opponent's waning arsenal...
http://www.quackometer.net/blog/2007/05/wi-fi-quackery-and-parliament.html0 -
I'll take two0
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No, this is absolute garbage. The wavelength of light that is needed to damage DNA lies in the higher energy regions of the electromagnetic spectrum, the higher end of the Ultra-violet (10 x 10^-9 m to 400 x 10^-9 m), the X-Ray (0.01 x 10^-9 to 10 x 10^-9 m), or the Gamma (< 0.02 x 10^-9 m).
Microwave light lies in the low energy region of the electromagnetic spectrum, or 1 mm to 1 m.
Furthermore, the photon energy required to break one of the chemical bonds of DNA, if we use the canonical equations relating the wavelength of light to the energy of a photon:
E = hν
where E is the energy (J, Joules which is a unit of energy), h is Plank's Constant (6.626 × 10-34 J s), and ν is the frequency (s^-1) of the wavelength of light. The frequency is also expressed in terms of the wavelength
ν= c/λ
where c is the speed of light (2.9979 x 10^8 m/s) and λ is the wavelength of light (in meters, m).
So, the energy for a photon is
E = hc/λ
Plugging in the values for the speed of light, Plank's constant, and the higher end of the Microwave region, or 1 mm (1 x 10^-3 m), the energy of a photon is
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (1 x 10^-3 m) = 1.986 x 10^-22 J
Similarly, the energy of a photon in the lower and upper regions of the Electromagnetic spectrum are
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (400 x 10^-9 m) = 4.966 x 10^-19 J
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (10 x 10^-9 m) = 1.986 x 10^-17 J.
The bond dissociation energy, or the energy required to break the covalent bonds (the class of bond that exists between all of the atoms in DNA). The most common bonds are carbon-hydrogen (C-H), carbon-carbon (C-C), and carbon-nitrogen (C-N) with bond energies 413, 348, and 308 kJ/mol, respectively ( a mol means 6.022 x 10^23 constituent particles or atoms per mol; a mol is a unit).
So, the energy in the weakest bond (in this case the carbon-nitrogen bond is
E = (308 x 10^3 J/mol)/(6.022 x 10^23 mol^-1) = 5.115 x 10^-19 J
THEREFORE, you need to be in the Ultra-violet region of the electromagnetic spectrum.
Logic! :noway:
We don't need no stinkin' logic!
(WTG! I knew this was true, but could never do the math to explain it.)0 -
I ran across this topic a couple of months ago. According to the article, Russia, and a few other countries I think, have outlawed using microwave ovens for food preparation.
I cannot speak to the safety of foods cooked in a microwave oven but I will state I prefer foods cooked by conventional methods; they just taste better. Even a simple baked potato, cooked in a conventional oven, tastes better and seems to have a better texture than those having been "nuked."0 -
No, this is absolute garbage. The wavelength of light that is needed to damage DNA lies in the higher energy regions of the electromagnetic spectrum, the higher end of the Ultra-violet (10 x 10^-9 m to 400 x 10^-9 m), the X-Ray (0.01 x 10^-9 to 10 x 10^-9 m), or the Gamma (< 0.02 x 10^-9 m).
Microwave light lies in the low energy region of the electromagnetic spectrum, or 1 mm to 1 m.
Furthermore, the photon energy required to break one of the chemical bonds of DNA, if we use the canonical equations relating the wavelength of light to the energy of a photon:
E = hν
where E is the energy (J, Joules which is a unit of energy), h is Plank's Constant (6.626 × 10-34 J s), and ν is the frequency (s^-1) of the wavelength of light. The frequency is also expressed in terms of the wavelength
ν= c/λ
where c is the speed of light (2.9979 x 10^8 m/s) and λ is the wavelength of light (in meters, m).
So, the energy for a photon is
E = hc/λ
Plugging in the values for the speed of light, Plank's constant, and the higher end of the Microwave region, or 1 mm (1 x 10^-3 m), the energy of a photon is
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (1 x 10^-3 m) = 1.986 x 10^-22 J
Similarly, the energy of a photon in the lower and upper regions of the Electromagnetic spectrum are
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (400 x 10^-9 m) = 4.966 x 10^-19 J
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (10 x 10^-9 m) = 1.986 x 10^-17 J.
The bond dissociation energy, or the energy required to break the covalent bonds (the class of bond that exists between all of the atoms in DNA). The most common bonds are carbon-hydrogen (C-H), carbon-carbon (C-C), and carbon-nitrogen (C-N) with bond energies 413, 348, and 308 kJ/mol, respectively ( a mol means 6.022 x 10^23 constituent particles or atoms per mol; a mol is a unit).
So, the energy in the weakest bond (in this case the carbon-nitrogen bond is
E = (308 x 10^3 J/mol)/(6.022 x 10^23 mol^-1) = 5.115 x 10^-19 J
THEREFORE, you need to be in the Ultra-violet region of the electromagnetic spectrum.
Logic! :noway:
We don't need no stinkin' logic!
(WTG! I knew this was true, but could never do the math to explain it.)
Science math is WAY harder than accounting math! :laugh:
Microwave ovens really suck for some things (like boiling water), but are absolutely perfect for other things.(like re-biophoton-izing a day-old donut)0 -
^ This. I consider him about as unbiased and reliable an information source as Dr. Oz.Dr mercola can and should be disregarded entirely.
WOAH WOAH WOAH! Pump the brakes! Don't bring The Great Doctor Oz into this mess!
Wait raspberry ketones can make me lose weight?? A magic (and cheap) weightloss pill that works for everyone?! Sign me up!0 -
What's a microwave? I thought they were called Death Boxes now.
I agree... I was in the process of removing my death box because I saw on the internet how terrible these contraptions really are.... I may even throw away my lighter and resort to lighting fires via stick rubbing, at least till they prove the spark from the sticks is strictly cancer.0 -
Here and I thought biophotons were where Superman stored power from the yellow sun...0
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Go study heat extension, heat capacity, plank wavelength and energy. Then understand why you cannot be right.0
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No, this is absolute garbage. The wavelength of light that is needed to damage DNA lies in the higher energy regions of the electromagnetic spectrum, the higher end of the Ultra-violet (10 x 10^-9 m to 400 x 10^-9 m), the X-Ray (0.01 x 10^-9 to 10 x 10^-9 m), or the Gamma (< 0.02 x 10^-9 m).
Microwave light lies in the low energy region of the electromagnetic spectrum, or 1 mm to 1 m.
Furthermore, the photon energy required to break one of the chemical bonds of DNA, if we use the canonical equations relating the wavelength of light to the energy of a photon:
E = hν
where E is the energy (J, Joules which is a unit of energy), h is Plank's Constant (6.626 × 10-34 J s), and ν is the frequency (s^-1) of the wavelength of light. The frequency is also expressed in terms of the wavelength
ν= c/λ
where c is the speed of light (2.9979 x 10^8 m/s) and λ is the wavelength of light (in meters, m).
So, the energy for a photon is
E = hc/λ
Plugging in the values for the speed of light, Plank's constant, and the higher end of the Microwave region, or 1 mm (1 x 10^-3 m), the energy of a photon is
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (1 x 10^-3 m) = 1.986 x 10^-22 J
Similarly, the energy of a photon in the lower and upper regions of the Electromagnetic spectrum are
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (400 x 10^-9 m) = 4.966 x 10^-19 J
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (10 x 10^-9 m) = 1.986 x 10^-17 J.
The bond dissociation energy, or the energy required to break the covalent bonds (the class of bond that exists between all of the atoms in DNA). The most common bonds are carbon-hydrogen (C-H), carbon-carbon (C-C), and carbon-nitrogen (C-N) with bond energies 413, 348, and 308 kJ/mol, respectively ( a mol means 6.022 x 10^23 constituent particles or atoms per mol; a mol is a unit).
So, the energy in the weakest bond (in this case the carbon-nitrogen bond is
E = (308 x 10^3 J/mol)/(6.022 x 10^23 mol^-1) = 5.115 x 10^-19 J
THEREFORE, you need to be in the Ultra-violet region of the electromagnetic spectrum.
Is it just me, or is this hot?0 -
Here and I thought biophotons were where Superman stored power from the yellow sun...
Or Birdman.0 -
No, this is absolute garbage. The wavelength of light that is needed to damage DNA lies in the higher energy regions of the electromagnetic spectrum, the higher end of the Ultra-violet (10 x 10^-9 m to 400 x 10^-9 m), the X-Ray (0.01 x 10^-9 to 10 x 10^-9 m), or the Gamma (< 0.02 x 10^-9 m).
Microwave light lies in the low energy region of the electromagnetic spectrum, or 1 mm to 1 m.
Furthermore, the photon energy required to break one of the chemical bonds of DNA, if we use the canonical equations relating the wavelength of light to the energy of a photon:
E = hν
where E is the energy (J, Joules which is a unit of energy), h is Plank's Constant (6.626 × 10-34 J s), and ν is the frequency (s^-1) of the wavelength of light. The frequency is also expressed in terms of the wavelength
ν= c/λ
where c is the speed of light (2.9979 x 10^8 m/s) and λ is the wavelength of light (in meters, m).
So, the energy for a photon is
E = hc/λ
Plugging in the values for the speed of light, Plank's constant, and the higher end of the Microwave region, or 1 mm (1 x 10^-3 m), the energy of a photon is
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (1 x 10^-3 m) = 1.986 x 10^-22 J
Similarly, the energy of a photon in the lower and upper regions of the Electromagnetic spectrum are
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (400 x 10^-9 m) = 4.966 x 10^-19 J
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (10 x 10^-9 m) = 1.986 x 10^-17 J.
The bond dissociation energy, or the energy required to break the covalent bonds (the class of bond that exists between all of the atoms in DNA). The most common bonds are carbon-hydrogen (C-H), carbon-carbon (C-C), and carbon-nitrogen (C-N) with bond energies 413, 348, and 308 kJ/mol, respectively ( a mol means 6.022 x 10^23 constituent particles or atoms per mol; a mol is a unit).
So, the energy in the weakest bond (in this case the carbon-nitrogen bond is
E = (308 x 10^3 J/mol)/(6.022 x 10^23 mol^-1) = 5.115 x 10^-19 J
THEREFORE, you need to be in the Ultra-violet region of the electromagnetic spectrum.
Is it just me, or is this hot?
Not just you. It's hot. She's edumacated and stuff.0 -
No, this is absolute garbage. The wavelength of light that is needed to damage DNA lies in the higher energy regions of the electromagnetic spectrum, the higher end of the Ultra-violet (10 x 10^-9 m to 400 x 10^-9 m), the X-Ray (0.01 x 10^-9 to 10 x 10^-9 m), or the Gamma (< 0.02 x 10^-9 m).
Microwave light lies in the low energy region of the electromagnetic spectrum, or 1 mm to 1 m.
Furthermore, the photon energy required to break one of the chemical bonds of DNA, if we use the canonical equations relating the wavelength of light to the energy of a photon:
E = hν
where E is the energy (J, Joules which is a unit of energy), h is Plank's Constant (6.626 × 10-34 J s), and ν is the frequency (s^-1) of the wavelength of light. The frequency is also expressed in terms of the wavelength
ν= c/λ
where c is the speed of light (2.9979 x 10^8 m/s) and λ is the wavelength of light (in meters, m).
So, the energy for a photon is
E = hc/λ
Plugging in the values for the speed of light, Plank's constant, and the higher end of the Microwave region, or 1 mm (1 x 10^-3 m), the energy of a photon is
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (1 x 10^-3 m) = 1.986 x 10^-22 J
Similarly, the energy of a photon in the lower and upper regions of the Electromagnetic spectrum are
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (400 x 10^-9 m) = 4.966 x 10^-19 J
E = [(6.626 x 10^-34 Js)(2.9979 x 10^8 m/s)]/ (10 x 10^-9 m) = 1.986 x 10^-17 J.
The bond dissociation energy, or the energy required to break the covalent bonds (the class of bond that exists between all of the atoms in DNA). The most common bonds are carbon-hydrogen (C-H), carbon-carbon (C-C), and carbon-nitrogen (C-N) with bond energies 413, 348, and 308 kJ/mol, respectively ( a mol means 6.022 x 10^23 constituent particles or atoms per mol; a mol is a unit).
So, the energy in the weakest bond (in this case the carbon-nitrogen bond is
E = (308 x 10^3 J/mol)/(6.022 x 10^23 mol^-1) = 5.115 x 10^-19 J
THEREFORE, you need to be in the Ultra-violet region of the electromagnetic spectrum.
someone paid attention in Chem 1! *sends fr*0 -
Well if this is true than I guess anybody whose ever put one of those small microwave transcievers called a CELL PHONE up their ear is screwed.
lol0 -
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