P2O5+C=P+CO2 Электронный баланс

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вопрос

In this equation, we have the following electron transfers:

P2O5 + C --> P + CO2

The oxidation states of each element are as follows:

Phosphorus (P) in P2O5 is in the +5 oxidation state.Carbon (C) in C is in the 0 oxidation state.Phosphorus (P) in P is in the +3 oxidation state.Carbon (C) in CO2 is in the +4 oxidation state.

To balance the electron transfer in this reaction, we need to ensure that the number of electrons lost by the reducing agent (C) is equal to the number of electrons gained by the oxidizing agent (P2O5).

We start by writing the half-reactions for each element:
Oxidation: C --> CO2 (loses 4 electrons)
Reduction: P2O5 --> P (gains 2 electrons)

To balance the electron transfer, we need to multiply the reduction half-reaction by 2 and the oxidation half-reaction by 4 to equalize the number of electrons exchanged.

4C --> 4CO2 (loses 16 electrons)
2P2O5 --> 4P + 5O2 (gains 4 electrons)

Now the electron transfer is balanced, with C losing 16 electrons and P2O5 gaining 16 electrons.