The discussion revolves around balancing oxidation-reduction equations, specifically using the example of photosynthesis. Participants are exploring the steps involved in balancing such equations and the complexities that arise compared to regular stoichiometric balancing.
Some guidance has been offered regarding the initial steps of balancing the equation, but there is a recognition that balancing redox reactions is more complex than standard stoichiometry. Participants are encouraged to provide examples for further exploration.
There is an indication that the original poster is seeking a deeper understanding of redox reactions specifically, which may involve additional considerations beyond the basic balancing steps discussed.
Originally posted by arcnets
gigi9,
photosynthesis might be a good example. Let's start from
H2O + CO2 -> C6H12O6 + O2.
First step, let's add what we have.
Left-hand side: 2H + 3O + 1C.
Right-hand side: 12H + 8O + 6C. So the formula is not balanced.
As a first step, we should look for an element that appears only in one component on each side. This is carbon. So, to balance carbon, we have to use 6 molecules of carbon dioxide:
H2O + 6CO2 -> C6H12O6 + O2.
Let's add what we have.
Left-hand side: 2H + 13O + 6C.
Right-hand side: 12H + 8O + 6C.
Is there another element which appears only once on each side? Yes, hydrogen! So we better use 6 molecules of water:
6H2O + 6CO2 -> C6H12O6 + O2.
Left-hand side: 12H + 18O + 6C.
Right-hand side: 12H + 8O + 6C.
We can balance this by adding more oxygen on the RHS:
6H2O + 6CO2 -> C6H12O6 + 6O2.
Now it's balanced.