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When H₂SO₃ is converted into H₂SO₄ the change in the oxidation state of sulphur is from:

0 to +2

+2 to +4

+4 to +2

+4 t0 +6

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Explanation

(d) S⁴⁺ $\to$ S⁶⁺ + 2e

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In which of the following processes nitrogen is oxidised?

N $H_{4}^{+}$ $\to$ N₂

N $O_{3}^{-} \to$ NO

NO₂ $\to$ N $O_{2}^{-}$

NO₃ $\to$ N $H_{4}^{+}$

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Explanation

(a) 2N^3- $\to$ N₂O + 6e

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In which reaction is hydrogen acting as an oxidising agent?

With ioding to give hydrogen iodide

With lithium to give lithium hydride

With nitrogen to give ammonia

With sulphur to give hydrogen sulphide

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Explanation

(b) 2e + $H_{2}^{0} \to$ 2H^1-

Li $\to$ Li¹⁺+ e

H₂ is reduced and thus, oxidant.

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Fluorine is a strong oxidising agent because:

it has several isotopes

it is very small and has 7 electrons in valency shell

its valency is one

it is the first member of the halogen series

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Explanation

(b) Due to smallest halogen, it possesses maximum tendency for accepting electron in aqueous medium.

(1/2) F₂+e+aq $\to$ F^-, $∆ H$ =-ve(max.for F₂)

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The oxidation state of Ni in Ni(CO)₄ is:

zero

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Explanation

(a) Ox. no. of Ni is equal to zero.

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Milliequivalents of a solute in a solution can be given by:

Mzeq_. = M x V_{in mL}

Meq. = N x V_{in mL}

Mzeq. = $\frac{m a s s}{E q . m a s s} \times$ 1000

both (b) and (c)

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Explanation

(d) These are formulae of Meq.

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HBr and HI reduce H₂SO₄, HCl can reduce KMnO₄ and HF can reduce:

H₂SO₄

K₂Cr₂O₇

KMnO₄

none of these

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Explanation

(d) F^- can be oxidised to F₂ only by electroysis.

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Sulphurous acid can be used as:

oxidising agent

reducing agent

bleaching agent

all of these

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Explanation

(d) S in H₂SO₃ is in +4 oxidation state. It lies in between its maximum and minimum oxidation state, i.e., +6 and -2 and thus, S can increase or decrease its ox. no. as the case may be.

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When SO₂ is passed through acidified solution of potassium dichromate, then chromium sulphate is formed. The change in oxidation number of chromium is:

+4 to+2

+5 to+3

+6 to+3

+7 to+2

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Explanation

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In which transfer of five electrons takes place?

Mn $O_{4}^{-}$ $\to$ Mn²⁺

Cr $O_{4}^{2 -}$ $\to$ Cr³⁺

Mn $O_{4}^{-}$ $\to$ MnO₂

Cr₂ $O_{7}^{2 -}$ $\to$ 2Cr³⁺

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Explanation

(a) Mn⁷⁺ + 5e $\to$ Mn²⁺

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