Which reagent oxidizes the ferrous oxalate dehydrate?
My crystal ball is hazy today. What are you doing? Which reagents are you using? I assume it's a typo but I'm sure you meant "dihydrate">
yes I think so I just am having trouble with chemistry this is hard
To determine which reagent oxidizes ferrous oxalate dehydrate, you need to understand the properties of the compound and identify potential oxidizing agents.
Ferrous oxalate dihydrate has the chemical formula FeC2O4 · 2H2O. It contains the iron (Fe) ion in the +2 oxidation state. Oxidization involves the gain of oxygen or the loss of electrons, resulting in an increase in the oxidation state of an element.
In order to oxidize ferrous oxalate dihydrate, you need to find a reagent that can facilitate the transfer of electrons from Fe(II) to Fe(III). This will cause the iron ion to be oxidized from +2 to +3.
One commonly used reagent for this purpose is potassium permanganate (KMnO4). Potassium permanganate is a strong oxidizing agent that can readily accept electrons. In an acidic medium, it can cause the Fe(II) ions in ferrous oxalate dihydrate to be oxidized to Fe(III) ions:
10FeC2O4 · 2H2O + 2KMnO4 + 8H2SO4 → 5Fe2(SO4)3 + 2MnSO4 + 10CO2 + 8H2O + K2SO4
In this reaction, the Mn(VII) in potassium permanganate is reduced to Mn(II), while the Fe(II) is oxidized to Fe(III) and gets converted to ferric sulfate (Fe2(SO4)3).
Therefore, potassium permanganate is the reagent that can effectively oxidize ferrous oxalate dihydrate.