Does the oxidation number of an element in any molecule or any polyatomic ion represent the actual charge on it?

What are the net charges on the left and right side of the following equations?Add electrons as necessary to make each of them balanced half reactions
CI₂ +4 H₂O \(\rightarrow\) 2CISO^-₂ +8H⁺

Nitric acid is an oxidising agent and reacts with Pbo but it does not react woth pbo₂ . Explain why?

Consider the reactions,
\({ C }_{ 6 }{ H }_{ 5 }CHO(l)+2{ Cu }^{ 2+ }(aq)+5{ OH }^{ - }(aq)\longrightarrow NO \ change \ observed.\)
What inference do you draw about the behaviour of Ag⁺ and Cu²⁺ from these reactions?

How many millimoles of potassium dichromate is required to oxidise 24mL of 0.5 M Mohr's salt solution in acidic medium?

Write the anode reaction, the cathode reaction and the net cell reaction in the following cells. Which electrode would be positive terminal in each cell?
Zn(s) \(|\) Zn²⁺|| Br₂ |Br^-| Pt(s)

Predict the products of electrolysis in each of the following:
(i) An aqueous solution of AgNO₃ with silver electrodes
(ii) An aqueous solution AgNO₃ with platinum electrodes
(iii) A dilute solution of H₂SO₄ with platinum electrodes
(iv) An aqueous solution of CuCl₂ with platinum electrodes

Using the standard electrode potentials given in the Table B.l, predict if the reaction between the following is feasible - Br₂ (aq) and Fe²⁺(aq)

Identify the oxidant and reductant in each of the following reactions.
(a) MnO^-₄ (aq) + C₂H₅OH(aq) \(\rightarrow \) Mn² + (aq) + CH₃COOH(aq)
(b) Zn(s) + 2H⁺(aq) → pb(s) + CO(g)
(c) pbO(s) + C(s) → pb(s) + CO(g)

Write the half reactions for the following redox reactions.
2K(s) + Cl₂(g)\(\rightarrow \)2Kcl(s)

Justify that the following reaction are redox reaction
\(4N{ H }_{ 3 }(g)+5{ O }_{ 2 }(g)\longrightarrow 4NO(g)+6H_{ 2 }O(g)\)