✓✗Tribromooctaoxide, Br₃O₈, is a neutral molecule. Its correct structure is

✓✗In the reaction H₂S + Cl₂ → 2HCl + S, the substance oxidised is

✓✗In the reaction 2Na + Cl₂ → 2NaCl, sodium is

✓✗In a disproportionation reaction,

✓✗According to the electronic concept, reduction is

✓✗Balance: MnO₄⁻ + C₂O₄²⁻ + H⁺ → Mn²⁺ + CO₂ + H₂O. The total of all coefficients in the balanced equation (smallest whole numbers) is

✓✗Arsenic(III) sulphide, As₂S₃, is oxidised by nitric acid to H₃AsO₄ and SO₄²⁻, with NO as the reduction product. The total number of electrons lost per As₂S₃ unit is

✓✗Statement I: Oxidation number of Cr in CrO₅ is +10.
Statement II: CrO₅ contains two peroxide linkages.

✓✗Consider the change in oxidation state of bromine corresponding to the different emf values shown below:
BrO₄⁻ \( \xrightarrow{\;1.82\,V\;} \) BrO₃⁻ ; BrO₃⁻ \( \xrightarrow{\;1.5\,V\;} \) HBrO ; HBrO \( \xrightarrow{\;1.595\,V\;} \) Br₂ ; Br₂ \( \xrightarrow{\;1.0652\,V\;} \) Br⁻
The species undergoing disproportionation is

✓✗The oxidation state of I in H₄IO₆⁻ is

✓✗Statement I: In the ion-electron method, the two half-reactions are multiplied so that the electrons lost equal the electrons gained.
Statement II: A balanced redox equation must be balanced for both atoms and charge.

✓✗Ozone acts as an oxidising agent in O₃ + 2KI + H₂O → 2KOH + I₂ + O₂. The species oxidised is

✓✗The number of moles of K₂Cr₂O₇ needed to oxidise 6 mol of Fe²⁺ in acidic medium is

✓✗Assertion: Fluorine does not show disproportionation.
Reason: Fluorine, being the most electronegative element, cannot show a positive oxidation state.

✓✗A metal M forms M³⁺ and is oxidised by K₂Cr₂O₇ from M²⁺. How many moles of M²⁺ are oxidised by 0.5 mol of K₂Cr₂O₇?