Redox Reactions · Chemistry · JEE Advanced

A sample (5.6 g) containing iron is completely dissolved in cold dilute HCl to prepare a 250 mL of solution. Titration of 25.0 mL of this solution requires 12.5 mL of 0.03 M KMnO₄ solution to reach the end point. Number of moles of Fe²⁺ present in 250 mL solution is x $$\times$$ 10^$$-$$2 (consider complete dissolution of FeCl₂). The amount of iron present in the sample is y% by weight.

(Assume : KMnO₄ reacts only with Fe²⁺ in the solution

Use : Molar mass of iron as 56 g mol^$$-$$1)

The value of x is ______.

A sample (5.6 g) containing iron is completely dissolved in cold dilute HCl to prepare a 250 mL of solution. Titration of 25.0 mL of this solution requires 12.5 mL of 0.03 M KMnO₄ solution to reach the end point. Number of moles of Fe²⁺ present in 250 mL solution is x $$\times$$ 10^$$-$$2 (consider complete dissolution of FeCl₂). The amount of iron present in the sample is y% by weight.

(Assume : KMnO₄ reacts only with Fe²⁺ in the solution

Use : Molar mass of iron as 56 g mol^$$-$$1)

The value of y is ______.

Ozonolysis of ClO₂ produces an oxide of chlorine. The average oxidation state of chlorine in this oxide is __________.

In neutral or faintly alkaline solution, 8 moles of permanganate anion quantitative oxidise thiosulphate anions to produce X moles of a sulphur containing product. The magnitude of X is....

Consider the following list of reagents, acidified K₂Cr₂O₇, alkaline KMnO₄, CuSO₄, H₂O₂, Cl₂, O₃, FeCl₃, HNO₃ and Na₂S₂O₃. The total number of reagents that can oxidise aqueous iodide to iodine is

The difference in the oxidation numbers of the two types of sulphur atoms in Na₂S₄O₆ is

Choose the correct statement(s) among the following :

For the reaction,

$${I^ - } + ClO_3^ - + {H_2}S{O_4} \to C{l^ - } + HSO_4^ - + {I_2}$$

the correct statement(s) in the balanced equation is/are

The order of the oxidation state of the phosphorous atom in

$${H_3}P{O_2},{H_3}P{O_4},{H_3}P{O_3}$$ and $${H_4}{P_2}{O_6}$$ is

The reaction, $$3Cl{O^ - }(aq)$$$$ \to ClO_3^ - (aq) + 2C{l^ - }(aq)$$ is an example of :

Amongst the following identify the species with an atom in +6 oxidation state

The normality of 0.3 M phosphorus acid (H₃PO₃) is

For the redox reaction:
$$MnO_4^ - + {C_2}O_4^{ - 2} + {H^ + }$$ $$ \to M{n^{2 + }} + C{O_2} + {H_2}O$$
The correct coefficients of the reactants for the balanced reaction are

The volume strength of 1.5 N H₂O₂ solution is

The oxidation number of phosphorus in Ba(H₂PO₂) is :

The equivalent weight of MnSO₄ is half of its molecular weight, when it converts to

The oxidation number of carbon in CH₂O is

1 mole of N₂H₄ loses 10 moles of electrons to form a new compound Y. assuming that all nitrogen appears in the new compound , what is the oxidation state of nitrogen in Y ? (there is no change in the oxidation state of hydrogen)

M is molecular weight of KMnO₄. The equivalent wight of KMnO₄ when it is converted into K₂MnO₄ is

To a 25ml H₂O₂ solution, excess of acidified solution of potassium iodide was added. The iodine liberated required 20 ml of 0.3 N sodium thiosulphate solution. Calculate the volume strength of H₂O₂ solution.

A 5.0 cm³ solution of H₂O₂ liberates 0.508 g of iodine from an acidified KI solution. Calculate the strength of H₂O₂ solution in terms of volume strength at STP.

Complete and balance the following equation:

S + OH^- $$\to$$ S^2- + $$S_2O_3^-$$

Arrange the following in increasing oxidation number of iodine.

I₂, HI, HIO₄, ICl

Complete and balance the following equation:

Ag⁺ + AsH₃ $$\to$$ H₃AsO₃ + H⁺

Complete and balance the following equation:

$$ClO_3^-$$ + I^- + H₂SO₄ $$\to$$ Cl^- + $$HSO_4^-$$

Complete and balance the following equation:

Mn²⁺ + PbO₂ $$\to$$ $$MnO_4^-$$ + H₂O

Complete and balance the following equations:

Cl₂ + OH^- $$\to$$ Cl^- + ClO^-

Complete and balance the following equation:

$$Cr_2O_7^{2-}$$ + C₂H₄O $$\to$$ C₂H₄O₂ + Cr³⁺

Complete and balance the following equation:

Zn + $$NO_3^- \to$$ Zn²⁺ + $$NH_4^+$$

Complete and balance the following equation:

Ce³⁺ + $$S_2O_8^{-2} \to $$ $$SO_4^{-2}$$ + Ce⁴⁺

Complete and balance the following equation:

HNO₃ + HCl $$\to$$ NO + Cl₂

Balance the following Equations:

(i) Cu₂O + H⁺ + $$NO_3^ - \to $$ Cu²⁺ + NO + H₂O

(ii) K₄[Fe(CN)₆] + H₂SO₄ + H₂O $$\to$$ K₂SO₄ + FeSO₄ + (NH₄)₂SO₄ + CO

(iii) C2H5OH + I₂ + OH^- $$\to$$ CHI₃ + $$HCO_3^-$$ + I^- + 4H₂O