Which of the following about photosynthetic light reactions in plants is false? And the answer is that the ultimate electron acceptor is O2, right? No. I mean, first of all, we can have cyclic electron flow like the next question is going to deal with. Additionally, the ultimate electron acceptor, if anything, would be NADP+ because it's going to get reduced to NADPH and carry those electrons to the Calvin cycle. Now, cyclic electron flow produces ATP but it does not produce oxygen and NADPH. Right? The ferredoxin is not taking the electrons to produce NADPH. It's bringing it back to the proton pump and no oxygen is produced because cyclic electron flow involves photosystem 1, not photosystem 2. And it's photosystem 2 where water is split and oxygen is released.
Now, archaea have redoxins which use light to generate a proton motive force, but rhodopsins are not limited to this function. I mean, we have rhodopsins in our eyes that have been modified for visual sensation. We also have seen rhodopsins that can be used as chloride pumps.
Now, in the chloroplast membrane, a photosystem contains many chlorophyll molecules which mainly transfer excited states to the reaction center chlorophyll. That is the main job. It’s like an antenna in the light-harvesting complex, focusing all that excitation on the reaction center to use an equation here that involves Planck’s constant (h) and c, which is the speed of light. So this is the Planck-Einstein equation. And to plug in our values:
E = h · c λWe're going to multiply \( h = 6.62607015 \times 10^{-34} \) joules·seconds by \( c = 3 \times 10^{8} \) meters/second, all over \( \lambda = 680 \) nanometers. Be careful here. Don't forget to convert your units when you solve this through. And if you solve this through, what you should wind up with is \( E = 2.925 \times 10^{-19} \) joules. This equation is just giving us the energy of one photon. We are asked for a mole, right? So we need to take that number \( 2.925 \times 10^{-19} \) and multiply it by Avogadro's number \( 6.022 \times 10^{23} \) to get the energy for a mole of photons. So that is going to give us about \( 176 \) kilojoules. More precisely, it's \( 176,144 \) joules per mole. So that would be equivalent to 176 kilojoules per mole.
Alright. Let's flip the page and finish this up.