NEET Chemistry Redox Reactions Class 11 Questions

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

Which of the following is not a redox reaction?

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?

What is the oxidation number of an element in its free or uncombined state?

What is the oxidation number of an element in its free or uncombined state?

What is the first step in balancing a redox reaction?

What is the standard electrode potential (E°) of the hydrogen electrode?

What is the standard electrode potential (E°) of the hydrogen electrode?

What does the oxidation number denote in a compound?

What is one of the half-reactions that indicates the oxidation process involving sodium?

In Stock notation, how is the oxidation number of a metal represented in a compound?

In balancing redox reactions, how do you equalize the number of electrons in the half-reactions?

In the half reaction 2 Na (s) → 2 Na+ (g) + 2e-, what is being oxidized?

What type of reaction is exemplified by the conversion of H3PO2 to H3PO4 in the presence of AgNO3?

What is the purpose of multiplying the oxidation half-reaction by 3 and the reduction half-reaction by 2 in the balancing of a redox reaction?

In the reaction 2Fe(s) + 3H2O(l) → Fe2O3(s) + 3H2(g), which substance is being oxidized?

In the reaction H3PO2(aq) + 4 AgNO3(aq) + 2 H2O(l) → H3PO4(aq) + 4Ag(s) + 4HNO3(aq), what is being reduced?

What is the standard electrode potential (E°) of the hydrogen electrode?

What is the standard electrode potential (E°) of the hydrogen electrode?

In a disproportionation reaction, an element in one oxidation state is simultaneously what?

What is the half-reaction for the oxidation of sodium in a redox reaction?

What is the standard electrode potential (E°) of the hydrogen electrode?

In the reaction 2Cl2(g) + 2Br–(aq) → 2Cl–(aq) + Br2(l), which species is being reduced?

What is the standard electrode potential (E°) of the hydrogen electrode?

Which of the following statements about balancing redox reactions is correct?

Which of the following combinations correctly identifies the species undergoing oxidation and reduction in the provided redox reactions?

Which of the following statements about oxidation numbers is correct?

Which of the following statements regarding oxidation numbers is correct?

Which of the following combinations regarding oxidation numbers is correct?

Which of the following statements about Standard Electrode Potential is correct?

Which of the following statements about standard electrode potential is correct?

Which of the following statements about oxidation numbers is correct?

Consider the following statements regarding oxidation numbers: 1) The oxidation number of an element in its free state is always zero. 2) In a molecule with multiple atoms of the same element, the oxidation number is the average of all atoms. 3) The more electronegative element in a bond always has a positive oxidation number. 4) The oxidation number can be negative in certain compounds. Which combination of these statements is correct?

Which of the following statements about oxidation numbers is correct?

Which of the following combinations correctly describes the steps involved in balancing redox reactions?

Which of the following statements about standard electrode potential is correct?

Which of the following statements about standard electrode potential are correct?

Which of the following statements about oxidation numbers is correct?

Which of the following statements about oxidation numbers is correct?