namata99
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Hello, I would need with this task:
Write a balanced equation for the oxidation of dissolved H2S to sulfate by dissolved oxygen. Indicate the oxidation states of the redox-sensitive elements involved.
- For each redox couple, write the oxidized and reduced species in an equation and balance the amount of element, except H and O.
- Balance electroneutrality by adding electrons.
- Balance the number of oxygen atoms by adding H2O.
- Balance the number of protons (H) by adding H+.
- Subtract the two half-reactions, canceling electrons to obtain the complete redox reaction.
Sulfide to Sulfate: H2S ->SO4 2-
Im not sure which are the redox couples and where to add electrons, but I've got this so far:
H2S + 1/2O2 -> S0 + H2O
S0 + 1 1/2O2 + H2O -> SO4 2- + 2H+
Can someone provide his advice or comment if this is correct and how to proceed further? Thanks!
Write a balanced equation for the oxidation of dissolved H2S to sulfate by dissolved oxygen. Indicate the oxidation states of the redox-sensitive elements involved.
- For each redox couple, write the oxidized and reduced species in an equation and balance the amount of element, except H and O.
- Balance electroneutrality by adding electrons.
- Balance the number of oxygen atoms by adding H2O.
- Balance the number of protons (H) by adding H+.
- Subtract the two half-reactions, canceling electrons to obtain the complete redox reaction.
Sulfide to Sulfate: H2S ->SO4 2-
Im not sure which are the redox couples and where to add electrons, but I've got this so far:
H2S + 1/2O2 -> S0 + H2O
S0 + 1 1/2O2 + H2O -> SO4 2- + 2H+
Can someone provide his advice or comment if this is correct and how to proceed further? Thanks!