So, if photosynthesis can't use all wavelengths, you're saying that plants growing isn't a decrease in entropy? Show us that. Preferably after the first question you dodged.
The total energy in the immediate surroundings is less than the energy that is available to be used to "push" the Endergonic process for forming glucose.
hint:
During
formation of glucose the system is gaining energy – so Δ
G is positive – Endergonic, non-spontaneous. To occur at all it must be “pushed or pulled” by associative Exergonic reaction – energy input from its surroundings.
Endergonic reactions can be achieved if they are either
pulled or
pushed by an
exergonic (stability increasing, negative change in
free energy) process. Of course, in all cases the net reaction of the
total system (the reaction under study plus the puller or pusher reaction) is exergonic.
All physical and chemical systems in the universe follow the
second law of thermodynamics and proceed in a downhill, i.e.,
exergonic, direction. Thus, left to itself, any physical or chemical system will proceed, according to the second law of thermodynamics, in a direction that tends to lower the
free energy of the system (Δ
G is negative), and thus to expend energy in the form of work.
The
energy transfer available in the immediate surrounding (proximity - touching the plant) when combined with the reaction for forming glucos is still a net increase in entropy
And of course - when a photosystem absorbs a photon, the internal energy (
U =
hν0) of the photon is converted into the free energy of the chlorophyll excited state (Δ
G)
and some part of the energy is expected to be converted into entropy (ΔS),
===========================================
- Photosystem I, non-cyclic electron flow path:
2Chlorophyll + 2γ(700 nm) -> 2Chlorophyll + NADPH + ATP+ H 2 O
cyclic electron flow path:
2Chlorophyll + 2γ(700 nm) -> 2Chlorophyll + ATP+ H 2 O
- Photosystem II:
H 2 O + 2γ(680 nm) + 2Chlorophyll -> 2Chlorophyll + 1/2 O 2 + 2H+
- Calvin Cycle:
6CO 2 + 12NADPH + 18ATP + 12H 2 O -> C 6 H 12 O 6
===================In summary -
PII - Photosystem II:
PI - Photosystem I:
12 PII + 12PI(non-cyclic) + 6PI(cyclic) + Calvin Cycle
give us
6CO 2 + 24H 2 O + 60γ -> C 6 H 12 O 6 + 6O 2 + 18H 2 O.
"We can of course see now how the biome functions thermodynamically. It requires a great deal of energy input in the form of light, and the
cumulative generation of entropy, first during the photosynthesis of glucose, and then through the respiration of glucose back into carbon dioxide and water (not to mention all of the other processes of life which go into circulating glucose through the biome) guarantees that the entropy always increases.
This relentless increase in entropy, along with the
conservation of energy (in terms of heat, internal energy and work) make up the two "laws" of thermodynamics."
A "decrease in entropy" for what? the reaction AND its immediate environment?
That answer that is always - "no".
That is demonstrably incorrect. We can measure the energy of the surroundings, and control for it, demonstrating how much is needed for photosynthesis. Not only is there sufficient energy in full daylight, but the excess is so great that plants have to adapt when exposed to too much of it like human tanning.
You seem to have missed the point entirely.
ΔStotal = ΔSsys + ΔSsurr
The increase in entropy - is specific to energy transfer to the plant based on the energy immediately available at the point of the skin of the plant. Chlorophyll reflects green light - none of that light is used by the plant. So you have energy applied to "push" the non-spontaneous Endergonic reaction sequence needed to make glucose. AT each stage as the effort is made to "roll uphill" a lot of energy is applied and some of it not used at all because the state of the system itself requires it.
Endergonic reactions can be achieved if they are either
pulled or
pushed by an
exergonic (stability increasing, negative change in
free energy) process. Of course,
in all cases the net reaction of the total system (the reaction under study plus the puller or pusher reaction) is
exergonic.
Exergonic means that ΔG is negative - the total system has lost energy because you "never get something for nothing"..
ΔG = ΔH – TΔS