Redox Reaction Questions

Standard reduction potentials of the half reactions are given below: F2(g) + 2e− → 2F− (aq); E° = +2.85V Cl2(g) + 2e− → 2Cl− (aq); E° = +1.36V Br2(l) + 2e− → 2Br− (aq); E° = +1.06V I2(s) + 2e− → 2I− (aq); E° = +0.53V The strongest oxidizing agent is;

Given below are two statements: Statements I: A negative E° means that the redox couple is a stronger reducing agent than the H+/H2. Statements II: A positive E° means that the redox couple is a weaker reducing agent than the H+/H2.

In the reaction, 4Fe + 3O2 → 2Fe2O3, which of the following statements in incorrect?

Which of the following represents a correctly balanced half reaction?

Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R): Assertion (A) : Oxidation involves gain of electrons and reduction involves loss of electrons. Reason (R): The overall reaction in which oxidati

Identify the species undergoing oxidation in the given reaction; H2S(g) + Cl2(g) → 2HCl(g) + S(g)

The conversion of sugar C12H22O11 → CO2 is;

The oxidation number of phosphorus varies from;

For the reaction given below, which statement is correct? 2Fe + 3CdCl2 → 2FeCl3 + 3Cd

Which of the following does not behave as reducing agent? A. H2SO3 B. SO2 C. H2S D. HNO3 The correct options is/are;

In ionic equation, BiO3− + 6H+ + xe− → Bi3+ + 3H2O the value of x is;

In the reaction, H2S + H2O2 → S + 2H2O; (A) S is the oxidant. (B) H2O is the reductant (C) H2S is an oxidant and H2O2 is a reductant. (D) H2S is a reductant and H2O2 is an oxidant. The correct statement is;

Oxidation number of an element in its free state is;

The number of electrons lost or gained during the change, Fe + H2O → Fe3O4 + H2 is;

Reduction is a process which involves;

When sulphur dioxide is passed in an acidified K2Cr2O7 solution, the oxidation state of sulphur is changed from;

In the reaction What is the value of n?

Standard reduction electrode potentials of three metals A, B and C are +0.5V, –3.0V & –1.2V respectively. The decreasing order of reducing powers of these metals is;

In the reaction: Ag + H2SO4 → Ag2SO4 + H2O + SO2 Sulphuric acid acts as;

In all of its compounds, oxidation state of oxygen may vary from;

Reaction V2O5 + 5Ca → 2V + 5CaO can be classified as;

In which of the following compounds the oxidation number of carbon is maximum?

In the given redox reaction: Cr2O7^2− + Fe2+ → Fe3+ + Cr3+ 1 mol of Cr2O7^2− oxidises:

When a zinc rod is kept in a copper nitrate solution what happens?

Redox reaction is generally a/an;

An element which never has a positive oxidation number in any of its compound is;

CuSO4 + Zn → Cu + ZnSO4 is an example of;

The average oxidation state of Fe in Fe3O4 is:

Consider the following reaction: The values of x, y and z in the balanced chemical reaction are respectively;

Which of the following is a redox reaction?

Identify which of the following species cannot act as reducing agent?

Chlorine has +1 oxidation state in;

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.

Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R): Assertion (A): MnO2 can act as an oxidizing agent as well as reducing agent. Reason (R): Oxidation state of Mn in MnO2 lies between its highest

The correct order of electron releasing tendency of the given metals is;

Which of the following statements is correct about oxidation state of S in Na2S4O6?

Which of the following reactions is not a disproportionation reaction?

In the ionic equation:the n-factor of KBrO3 will be;

Oxidation state of P in PO4^3− is;

In C + H2O → CO + H2 ; H2O acts as: