Redox Reaction Questions
The number of moles of KMnO4 that will be needed to react completely with one mole of ferrous oxalate in acid solution is
The oxidation number of Sulphur in S₈ and S₂F₂ respectively are
Match the half-reactions (in column I) with change in oxidation number (in column II)
The number of oxygen atoms showing –1 oxidation state in CrO5 molecule are:
Which of the following is a redox reaction?
Given; Co3+ + e− → Co2+ ; E° = +1.81V Pb4+ + 2e− → Pb2+ ; E° = +1.67V Ce4+ + e− → Ce3+ ; E° = +1.61V Oxidizing power of the species will increase in the order:
–3 oxidation state of nitrogen will be obtained in case of;
2Na2O2 → 2Na2O + O2, is an example of disproportionation because:
The value of ‘n’ in the balanced reaction: will be;
In which of the following compounds, oxygen shows positive oxidation state?
In which of the following reactions H2O2 acts as a reducing agent?
A metal X displaces nickel from nickel sulphate solution but does not displace manganese from manganese sulphate solution. What is the correct order of their reducing powers?
Which of the following is the most powerful oxidising agent?
The oxidation state of Xe in Ba2XeO6 is:
In all of its compounds, oxidation state of oxygen may vary from;
Zero oxidation state is present in:
An element which never has a positive oxidation number in any of its compound is;
Arrange the following species in order of an increase in oxidation number of Mn; I. Mn2+ II. MnO2 III. KMnO4 IV. K2MnO4
In the reaction: Br2 + 6CO3^2− + 3H2O → 5Br− + BrO3− + 6HCO3−
Consider the following statements: (I) Addition of oxygen or electronegative element to a substance is called oxidation. (II) Electron donors act as reducing agent. (III) An oxidising agent accepts electrons. The correct statements are;
Given below are two statements: Statement I: Oxidation state of central Br in Br3O8 is +4. Statement II: Oxidation state of terminal Br in Br3O8 is +6. Choose the correct answer:
The oxidation number of phosphorus varies from;
Consider the following reaction; S + 12OH− → 4S^2− + 2S2O3^2− + 8H2O Which of the following is correct for the above reaction?
Oxidation state of middle carbon in C3O2 (Carbon suboxide) is;
The average oxidation state of Fe in Fe3O4 is:
Which of the following changes does not require only two electrons to occur?
Given below are two statements: Statements I: KMnO4 can work both as an oxidising as well as reducing agent. Statements II: The equation, Mg(s) + CuO(s) → MgO(s) + Cu(s) represents decomposition reaction. In the light of the above statements, choose
Zn rod is dipped in blue coloured solution of aqueous Cu(NO3)2. The incorrect statement among the following is;
The oxidation state of oxygen in the following reaction changes, K2O2 → KO2
Chlorine has +1 oxidation state in;
The equivalent weight of Fe^3+ (Molar mass = M g/mol) in the given reaction is: Fe^3+ + e− → Fe^2+
The oxidising agent in the following reaction is: S2O3^2− + I2 → S4O6^2− + 2I−
Given below are two statements: Assertion (A): In Na2O2, the oxidation state of each oxygen atom is –1. Reason (R): In peroxides, each oxygen atom is assigned an oxidation number of –1.
Given below are two statements: Statement I: The oxidation state of carbon in HCOOH is +2. Statement II: The oxidation state of nitrogen in N3H is –1/3. In the light of the above statements, choose the most appropriate answer:
Match List-I with List-II. List-I (Reactions) (A) Combination reaction (B) Decomposition reaction (C) Metal displacement reaction (D) Non-metal displacement reaction List-II (Examples) (I) Fe + 2HCl → FeCl2 + H2 (II) C + O2 → CO2 (III) Cr2O3 + 2Al →
The change in oxidation state of sulphur in the given reaction is from: PbS + 4H2O2 → PbSO4 + 4H2O
Consider the balanced reaction: The correct coefficient x, y and z are:
Match List-I with List-II. List-I (Molecule) (A) KO3 (B) H2O2 (C) MgO (D) KO2 List-II (Oxidation state of oxygen) (I) –1 (II) –1/3 (III) –1/2 (IV) –2 Choose the correct answer from the options given below:
The oxidation state of two terminal and two middle sulphur atoms in respectively are:
Which of the following can not act as reducing agent?
The species undergoing oxidation in the following reaction is: 3SO3^2− + Cr2O7^2− + 8H+ → 3SO4^2− + 2Cr^3+ + 4H2O
Match List-I with List-II. List-I (Compound) List-II (Average Oxidation state of central atom) A. H4P2O7 B. C3O4 C. H2S4O6 D. K2MnO4
Which of the following is not a redox reaction?
Cl2 changes to Cl− and ClO− in cold and dil. NaOH. The equivalent weight of Cl2 (molar mass = M) will be:
For the reaction, MnO4− + I− → MnO2 + I2 in basic medium, coefficients of I− and MnO4− in the balanced equation respectively are;
Identify in which of the following reaction(s), H2O2 is being oxidized and choose the correct option. A. H2O2 + 2H+ + 2e− → 2H2O B. H2O2 → O2 + 2H+ + 2e− C. H2O2 + 2e− → 2OH−
Given below are two statements: Statements I: In Br3O8 each of the two terminal bromine atoms are present in +6 oxidation state. Statements II: In Br3O8, the middle bromine is present in +4 oxidation state.
Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R): Assertion (A) : Equivalent weight of N2 in the reaction N2 + H2 → NH3 is 28/6. Reason (R): Equivalent weight = Molecular weight / number of e− l
–3 oxidation state of nitrogen will be obtained in case of;
Match List-I with List-II. List-I (Chemical Species) List-II (Oxidation no. of central atom) A. CrO5 B. I3− C. O3 D. F−