H₂S (g) + Cl₂ (g) → 2 HCl (g) + S (s)

The correct statement(s) in the balanced equation is(are):

a. H₂S is oxidised
b. Cl₂ is reduced
c. H₂S is reduced
d. Cl₂ is oxidised

1. a, b
2. b, c
3. c, d
4. a, d

2 Na(s) + H₂(g) → 2 NaH (s)

The incorrect statement among the following regarding above mentioned reaction is:

1. Na gets oxidised
2. It is a redox reaction
3. NaH is an ionic hydride
4. None of the above

Match the items in column I with column II.
(O.S = oxidation state)

2Cu₂O(s) + Cu₂S(s) → 6Cu(s) + SO₂(g)

The correct statement among the following regarding above mentioned reaction is:

1. Cu is reduced and Cu(I) is an reductant.
2. Sulphur is reduced and S in Cu₂S acts as oxidant.
3. Cu(I) is an oxidant and Cu(I) is reduced.
4. Sulphur is reduced and Cu is oxidised.

The species among the following that does not show a disproportionation reaction is-

ClO^–, ClO₂^–, \(ClO_{3}^{-}\) and ClO₄^–

1. ClO^–
2. ClO₂^–
3. ClO₄^–
4. \(ClO_{3}^{-}\)

Match the items in column I with the items in column II.

Consider the following reaction:

Pb₃O₄ + 8HCl → A +  B + 4H₂O

A and B are, respectively,:

1. A= PbCl₄;  B= PbCl₂
2. A= PbCl₂;  B= Cl₂ 
3. A= PbCl₄; B=Cl₂
4. A = PbCl₂; B = O₂

Consider the following equation:

Cr₂O₇^2–_(aq) + 3SO₃^2– _(aq)+ 8H⁺_(aq) →  A + B +4H₂O_(l)

The product A and B are respectively:

1. 2Cr²⁺; 3SO₂

2. 2Cr⁺; S₂O₇ ^2-

3. 2Cr³⁺; 3SO₄ ^2-

4. 2Cr³⁺; 3HSO₄^2-

 

Permanganate(VII) ion, MnO₄^– in basic solution oxidizes iodide ion, I^– to produce molecular iodine (I₂) and manganese (IV) oxide (MnO₂). The reaction is as follows:

aI^–(aq) + bMnO₄^–(aq) + cH₂O(l) → dI₂(s) + eMnO₂(s) + fOH^–(aq)

The value of b, d and f are-