What are the two half reactions for 3Mg+1Fe2(SO4)3 yields 3MgSO4+2Fe? thanks for your help
The half reactions in net ionic form are:
Mg --> Mg^+2 + 2e^- (oxidation)
Fe^+3 + 3e^- --> Fe (reduction)
To determine the half reactions for the given chemical equation, we need to split the equation into two separate reactions, one oxidation half reaction and one reduction half reaction.
Let's identify the oxidized and reduced species in the given reaction:
3Mg + 1Fe2(SO4)3 → 3MgSO4 + 2Fe
Oxidized species: The oxidation state of magnesium (Mg) increases from 0 to +2. Therefore, Mg is being oxidized.
Reduced species: The oxidation state of iron (Fe) decreases from +3 to 0. Therefore, Fe is being reduced.
Now, we can write the oxidation and reduction half reactions separately:
Oxidation Half Reaction: Mg → Mg2+ + 2e-
In this half reaction, magnesium (Mg) loses two electrons (e-) and is oxidized to form magnesium ions (Mg2+).
Reduction Half Reaction: Fe3+ + 3e- → Fe
In this half reaction, iron ions (Fe3+) gain three electrons (e-) and are reduced to form iron (Fe).
These half reactions can be balanced by adding the appropriate number of electrons and adjusting the coefficients if necessary.