NEET Chemistry Redox Reactions Class 11 Questions

Which of the following is not a redox reaction?

KMnO₄ acts as an oxidising agent in alkaline medium. When alkaline KMnO₄ is treated with KI, iodine is oxidised to

Which of the following reactions shows the reducing property of SO₂ ? (i) Cl₂ + SO₂ → SO₂Cl₂ (ii) 2H₂S + SO₂ → 3S + 2H₂O (iii) 2FeCl₃ + SO₂ + 2H₂O → 2FeCl₂ + H₂SO₄ + 2HCl (iv) SO₂ + H₂O → H₂SO₃

H₂O₂ + H₂O₂ → 2H₂O + O₂ is an example of disproportionation because:

The correct order of N⁻compounds in its decreasing order of oxidation states is

When KMnO₄ is reduced with oxalic acid in acidic solution, the oxidation number of Mn changes from

In the following questions, a statement of assertion is followed by a statement of reason. Mark the correct choice as: Assertion : Sn in +2 oxidation state is a reducing agent while Pb in +4 state is an oxidising agent. Reason : Inert pair effect is due to participation of s electrons in bond formation.

The values of coefficients to balance the following reaction are Cr(OH)₃ + ClO⁻ + OH⁻ → CrO₄²⁻ + Cl⁻ + H₂O

An example of a disproportionation reaction is

Assertion: KMnO₄, KClO₄, and HNO₃ act as oxidants. Reason: In KMnO₄, KClO₄ and HNO₃ central atom is in its highest oxidation state.

Identify disproportionation reaction

Given below are two statements. Statement I : Iron(III) catalyst, acidified K₂Cr₂O₇ and neutral KMnO₄ have the ability to oxidise I⁻ to I₂ independently. Statement II : Manganate ion is paramagnetic in nature and involves π-π bonding. In the light of the above statements, choose the correct answer from the options given below :

Which of the following colour changes shown during redox titrations is not correct?

Which of the following arrangements represent increasing oxidation number of the central atom?

Consider the following compounds: KO₂, H₂O₂ and H₂SO₄. The oxidation states of the underlined elements in them are, respectively,

Which reaction is NOT a redox reaction?

On balancing the given redox reaction, a Cr₂O₇²⁻ + b SO₃²⁻(aq) + c H⁺(aq) → 2a Cr³⁺(aq) + b SO₄²⁻(aq) + c/2 H₂O(ℓ) the coefficients a, b and c are found to be, respectively -

In the neutral or faintly alkaline medium, KMnO₄ oxidises iodide into iodate. The change in oxidation state of manganese in this reaction is from

Which of the following reactions is the metal displacement reaction? Choose the right option.

What is the change in oxidation number of carbon in the following reaction? CH₄(g) + 4Cl₂(g) → CCl₄(l) + 4HCl(g)

Which of the following reactions are disproportionation reactions?

The CORRECT order of N⁻compounds in its decreasing order of oxidation states is _______.

Consider the change in oxidation state of bromine corresponding to different emf values as shown in the diagram below: BrO₃⁻ \(\overset{1.82 \text{ V}}{\longrightarrow}\) BrO₂⁻ \(\overset{1.5 \text{ V}}{\longrightarrow}\) HBrO \(\overset{1.595 \text{ V}}{\longrightarrow}\) Br₂ \(\overset{1.0652 \text{ V}}{\longrightarrow}\) Br⁻ Then the species undergoing disproportionation is __________.

For the redox reaction, MnO₄⁻ + C₂O₄²⁻ + H⁺ ⟶ Mn²⁺ + CO₂ + H₂O the CORRECT coefficients of the reactants for the balanced reaction are

Name the gas that can readily decolourise acidified KMnO₄ solution. (A) SO₂ (B) NO₂ (C) P₂O₅ (D) CO₂

Which of the following statements is INCORRECT?

Which one of the following statements is CORRECT when SO₂ is passed through acidified K₂Cr₂O₇ solution?

Which of the following processes does NOT involve oxidation of iron?

The pair of compounds that can exist together is

In acidic medium, H₂O₂ changes Cr₂O₇²⁻ to CrO₅ which has two (O–O) bonds. Oxidation state of Cr in CrO₅ is

i. H₂O₂ + O₃ ⟶ H₂O + O₂ ii. H₂O₂ + Ag₂O ⟶ 2Ag + H₂O + O₂ Role of hydrogen peroxide in the above reactions is respectively

The reaction of aqueous KMnO₄ with H₂O₂ in acidic conditions gives