how do i calculate a concentration ratio of oxidised to reduced cytochrome c Fe2+ to Fe3+
given at 25 C and pH7
E(mV) as 100
and absorbance at 550nm as 1.5
E is relative to standard hydrogen electrode
i don't know how im supposed to calculate it from this data
please help!!!
To calculate the concentration ratio of oxidized (Fe3+) to reduced (Fe2+) cytochrome c, you can use the Nernst equation. The Nernst equation relates the electrode potential (E) to the concentration ratio of the oxidized and reduced species.
The Nernst equation is given as:
E = E° + (0.0592/n) * log([ox]/[red])
where:
- E is the electrode potential (in volts),
- E° is the standard electrode potential (in volts) (relative to the standard hydrogen electrode),
- n is the number of electrons transferred in the redox reaction,
- [ox] and [red] are the concentrations of the oxidized and reduced forms of cytochrome c, respectively (in molarity).
Given that you have the following information:
- E(mV) = 100 (relative to the standard hydrogen electrode)
- pH = 7 (pH does not directly affect the concentration ratio calculation)
- Absorbance at 550nm = 1.5 (although absorbance is not directly used in concentration calculations, it can be related to the concentration ratio indirectly)
It seems like you are missing some critical information to directly calculate the concentration ratio using the Nernst equation. Specifically, you would need the standard electrode potential (E°) and the number of electrons transferred (n) in the redox reaction.
Without these parameters, it would not be possible to calculate the concentration ratio accurately. I would suggest obtaining more information about the redox reaction involving cytochrome c to complete the calculation.