for the reaction, determine the number of transferring electrons so then i can pug into G=-nFE
I'm assigning charges to each of the elements
H2O2(aq) + 2ClO2(g) → O2(g) + 2HClO2(aq)
(+1,-1) + (+4,-2) (0) (+1,+1,-2)
since O changes from -1 to 0, so it lost one electron but Cl gains 3 electrons, so I'm confused is it a total of 3 electrons that are being transferred?
To determine the number of electrons being transferred in a redox reaction, you can follow these steps:
1. Assign oxidation numbers to all the elements in the reaction. This step helps you track the changes in the oxidation state of each element.
In this case:
H2O2(aq) + 2ClO2(g) → O2(g) + 2HClO2(aq)
The oxidation numbers are:
H2O2: H = +1, O = -1
ClO2: Cl = +4, O = -2
O2: O = 0
HClO2: O = -2, H = +1, Cl = +1
2. Compare the oxidation numbers to identify which elements are being oxidized (losing electrons) and which elements are being reduced (gaining electrons).
In our reaction:
- Oxygen (O) changes from -1 in H2O2 to 0 in O2. It gained two electrons and is reduced.
- Chlorine (Cl) changes from +4 in ClO2 to +1 in HClO2. It gained three electrons and is reduced.
Therefore, in total, three electrons are being transferred in the reaction:
2 electrons from oxygen (O) and 1 electron from chlorine (Cl).
Now, you can use this information to plug into the equation G = -nFE, where G is the Gibbs free energy change, n is the number of electrons, F is the Faraday's constant, and E is the cell potential.