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The following reaction takes place in an acidic solution. MnO4–(aq) + Cl–(aq) Mn2+ + Cl2(g) (unbalanced) Write the reduction and oxidation half-reactions (without electrons). :(?
Reduction Half-Reaction: MnO4-(aq) → Mn2+(aq) Oxidation Half-Reaction: Cl-(aq) → Cl2(g)
What is the balanced net ionic equation for the reaction between MnO4- ions and H2C2O4 in acid solution?
2MnO4- + 6H+ + 5(COOH)2 ----> 10CO2 + 2Mn2+ + 8H2O
Why KMnO4 titration's are carried out only in the presence of dilute H2SO4?
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.
What colour change occurs when h2o2 is added to kmno4?
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.
How many moles of Fe2 plus ion can be oxidized by 1.4x10-2 moles MnO4- ion?
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.
Overall redox equation fo MnO4 reacting with Fe2 in acid solution give Mn2 and Fe3?
8H+ + MnO4- + 5Fe2+--> 5Fe3+ + Mn2+ + 4H20
The following reaction takes place in an acidic solution. MnO4–(aq) + Cl–(aq) Mn2+ + Cl2(g) (unbalanced) Write the reduction and oxidation half-reactions (without electrons). :(?
Reduction Half-Reaction: MnO4-(aq) → Mn2+(aq) Oxidation Half-Reaction: Cl-(aq) → Cl2(g)
What is the balanced net ionic equation for the reaction between MnO4- ions and H2C2O4 in acid solution?
2MnO4- + 6H+ + 5(COOH)2 ----> 10CO2 + 2Mn2+ + 8H2O
Why KMnO4 titration's are carried out only in the presence of dilute H2SO4?
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.
What is the SPDF Notation for Mn2 plus?
Mn: 1s22s22p63s23p63d54s2 Mn2+: 1s22s22p63s23p63d5
What is the dissociation reaction for MnO 4?
In an acidic solution: 8 H+ + MnO4− + 5 e− → Mn2+ + 4 H2O In a neutral solution: 2 H2O + MnO4− + 3 e− → MnO2 + 4 OH−
What is the name of Mn2 plus ion?
The name of the Mn2+ ion is manganese(II) ion.
Complete redox reaction under acid condition MnO4 H2O2?
6H+(aq)+ 2MnO4-(aq)+ 5H2O2(l) ---> 2Mn2+(aq)+ 5O2(g) + 8H2O(l)
In the reaction Mg(s) plus 2H2O(I) and 61664 Mg(OH)2(s) plus H2(g) what is the oxidation state of each H in H2(g)?
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+.
Which balanced equation represents an oxidation-reduction reaction?
Equations that separate the oxidation from the reduction parts of the reaction
What colour change occurs when h2o2 is added to kmno4?
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.
How many moles of Fe2 plus ion can be oxidized by 1.4x10-2 moles MnO4- ion?
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.
