If I have 2- 1/2 reactions that are- O2(g)+4H(aq)+4e- -------2H2O and CyFe3+(aq) +e---------CyFe2+(aq) How do I determine the # of electrons transfered? In addition, if the electrons are on different sides of the equations how would I then determine the # being transfered? Thank you for looking at this!
For #1, the equation tells you 4 electrons are transferred and 1 electron transferred for #2.
To balance the two half reactions for a complete reaction, you will multiply half reaction 1 by 1 and half reaction 2 by 4, then add the two half reactions/equations. That will give you 4e on the left side of the arrow and 4e on the right side of the arrow which tells you (a) the electrons cancel and (b) there are 4 electrons transferred in the total reaction.
To determine the number of electrons transferred in a redox reaction, you need to consider the balanced half-reactions. In a balanced half-reaction, the number of electrons involved can be determined by looking at the coefficients of the species involved in the reaction.
Let's analyze the given half-reactions:
1) O2(g) + 4H+(aq) + 4e- → 2H2O
2) CyFe3+(aq) + e- → CyFe2+(aq)
In the first half-reaction, you have 4 electrons on the left side and none on the right side. This means that 4 electrons are being transferred in this oxidation half-reaction.
In the second half-reaction, you have 1 electron on the left side and none on the right side. This indicates that 1 electron is being transferred in this reduction half-reaction.
If the electrons are on different sides of the equation, you need to multiply the half-reactions by appropriate factors so that the number of electrons transferred is the same in both reactions. Once you have balanced the half-reactions, you can determine the number of electrons transferred by looking at the coefficients of the species involved in the reaction.
Remember that in a balanced redox reaction, the number of electrons gained in the reduction half-reaction must be equal to the number of electrons lost in the oxidation half-reaction.