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During the disproportionation of lodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is :

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Important Questions on Redox Reactions

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Beta Question Bank for Engineering: Chemistry>Chapter 6 - Redox Reactions>EXERCISE-2>Q 3

When $ZnS$ is boiled with strong nitric acid, the products are zinc nitrate, sulphuric acid and nitrogen dioxide. What are the changes in the oxidation numbers of $Zn, S$ and $N$ :

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Beta Question Bank for Engineering: Chemistry>Chapter 6 - Redox Reactions>EXERCISE-2>Q 4

${CN}^{-}$ is oxidised by ${NO}_{3}^{-}$ in the presence of an acid : ${aCN}^{-} + {bNO}_{3}^{-} + {cH}^{+} ⟶ (a + b) NO + {aCO}_{2} + \frac{c}{2} H_{2} O$ . What are the whole number values of $a, b, c$ in that order?

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Beta Question Bank for Engineering: Chemistry>Chapter 6 - Redox Reactions>EXERCISE-2>Q 5

Which of the following solutions will exactly oxidize $25 mL$ of an acid solution of $0.1 M$ iron $(II)$ oxalate?

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Beta Question Bank for Engineering: Chemistry>Chapter 6 - Redox Reactions>EXERCISE-2>Q 6

35 mL

sample of hydrogen peroxide gives off

500 mL

O_{2}

27^{\circ} C

and

1

atm

pressure. Determine volume strength of

H_{2} O_{2}

sample.

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Beta Question Bank for Engineering: Chemistry>Chapter 6 - Redox Reactions>EXERCISE-2>Q 8

The following reaction describes the rusting of iron,

4 Fe + 3 O_{2} ⟶ 4 {Fe}^{3 +} + 6 O^{2 -} .

Which one of the following statements are correct:

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Beta Question Bank for Engineering: Chemistry>Chapter 6 - Redox Reactions>EXERCISE-2>Q 12

A mixture of H₂SO₄ and H₂C₂O₄ (Oxalic acid) and some inert impurity weighing 3.185 g was dissolved in water and the solution made up to 1 litre, 10 mL of this solution required 3 mL of 0.1 N NaOH for complete neutralization. In another experiment, 100 mL of the same solution in hot condition required 4 mL of 0.02 M KMnO₄ solution for complete reaction. The wt. % of H₂SO₄ in the mixture was:

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Beta Question Bank for Engineering: Chemistry>Chapter 6 - Redox Reactions>EXERCISE-3>Q 14

1.0 g

sample of

{Fe}_{2} O_{3}

solid of

55.2 %

purity is dissolved in acid and reduced by heating the solution with zinc dust. The resultant solution is cooled and made up to

100.0 mL .

An aliquot of

25.0 mL

of this solution requires

17.0 mL

0.0167 M

solution of an oxidant for titration. Calculate the number of moles of electrons taken up by the oxidant in the reaction of the above titration.

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Beta Question Bank for Engineering: Chemistry>Chapter 6 - Redox Reactions>EXERCISE-3>Q 15

{KMnO}_{4}

oxidizes

X^{n +}

ion to

{XO}_{3}^{-},

itself changing to

{Mn}^{2 +}

in acid medium.

2.68 \times 10^{- 3}

mole

X^{n +}

requires

1.61 \times 10^{- 3}

mole

{MnO}_{4}^{-},

if the weight of

1 g

equivalent of

{XCl}_{n}

56 .

Report the value of

\frac{X}{n},

where

X

is the molar mass of

X^{n +} .

During the disproportionation of lodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is :

Important Questions on Redox Reactions

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