Oxidant half reaction: MnO4- + 8 H+ + 5e- --> Mn2+ + 4 H2O
Reduction Half-Reaction: MnO4-(aq) → Mn2+(aq) Oxidation Half-Reaction: Cl-(aq) → Cl2(g)
2MnO4- + 6H+ + 5(COOH)2 ----> 10CO2 + 2Mn2+ + 8H2O
The permanganate ion, MnO4- purple in colour. The sulfuric acid is added to create acidic conditions. In acidic conditions, the MnO4- gets reduced to Mn2+ which is colourless. Therefore, judging by the colour change, we can figure out how much of the potassium permanganate has been used.
When hydrogen peroxide (H2O2) is added to potassium permanganate (KMnO4), the purple color of KMnO4 solution fades, turning into a colorless solution. This color change indicates the reduction of KMnO4 to Mn2+ ions.
The molar mass of Fe2O3 is 55.845 (molar mass of iron)*2+16(molar mass of oxygen)*3, which comes out to be 159.69 grams per mole. Multiply that by the number of moles, and the answer is 223.57 grams.
8H+ + MnO4- + 5Fe2+--> 5Fe3+ + Mn2+ + 4H20
Reduction Half-Reaction: MnO4-(aq) → Mn2+(aq) Oxidation Half-Reaction: Cl-(aq) → Cl2(g)
2MnO4- + 6H+ + 5(COOH)2 ----> 10CO2 + 2Mn2+ + 8H2O
The permanganate ion, MnO4- purple in colour. The sulfuric acid is added to create acidic conditions. In acidic conditions, the MnO4- gets reduced to Mn2+ which is colourless. Therefore, judging by the colour change, we can figure out how much of the potassium permanganate has been used.
Mn: 1s22s22p63s23p63d54s2 Mn2+: 1s22s22p63s23p63d5
In an acidic solution: 8 H+ + MnO4− + 5 e− → Mn2+ + 4 H2O In a neutral solution: 2 H2O + MnO4− + 3 e− → MnO2 + 4 OH−
The name of the Mn2+ ion is manganese(II) ion.
6H+(aq)+ 2MnO4-(aq)+ 5H2O2(l) ---> 2Mn2+(aq)+ 5O2(g) + 8H2O(l)
Simply remember OIL RIG. Oxidation Is Loss (of electron) and Reduction Is Gain (of electron). In the case of MnO4-(aq) + 8H+(aq) + 5e- --> Mn2+(aq) + 4H2O(l) H is the oxidizing agent, because it causes Mn to be oxidized to Mn2+.
Equations that separate the oxidation from the reduction parts of the reaction
When hydrogen peroxide (H2O2) is added to potassium permanganate (KMnO4), the purple color of KMnO4 solution fades, turning into a colorless solution. This color change indicates the reduction of KMnO4 to Mn2+ ions.
The molar mass of Fe2O3 is 55.845 (molar mass of iron)*2+16(molar mass of oxygen)*3, which comes out to be 159.69 grams per mole. Multiply that by the number of moles, and the answer is 223.57 grams.