Middle of Pyramid - Test # 34

When a metal is burnt, its mass is increased by 24 percent. The equivalent mass of the metal will be:
1. 25
2. 24
3. 33.3
4. 76

The equivalent mass of H₃PO₄ in the following reaction is,
H₃PO₄+ Ca(OH)₂ $\to$ CaHPO₄ + 2H₂O
1. 98
2. 49
3. 32.66
4. 40

1.520g of the hydroxide of a metal on ignition gave 0.995 g of oxide. The equivalent mass of metal is:
1. 1.520
2. 0.995
3. 19.00
4. 9.00

What will be the normality of a solution obtained by mixing 0.45 N and 0.60 N NaOH in the ratio 2:1 by volume?
1. 0.4 N
2. 0.5 N
3. 1.05 N
4. 0.15 N

A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide have yielded 1.05g of the metal. We may deduce that:
1. the atomic mass of the metal is 8
2. the atomic mass of the metal is 4
3. the equivalent mass of the metal is 4
4. the equivalent mass of the metal is 8

An oxide of metal has 20% oxygen, the equivalent mass of oxide is:
1. 32
2. 40
3. 48
4. 52

A compound contains atoms of three elements A,B and C. If the oxidation number of A is +2, Bis +5 and that of C is -2, the possible formula of the compound is :
1. A₂(BC₃)₂
2. A₃(B₄C)₂
3. A₃(BC₄)₂
4. ABC₂

The number of peroxide linkages in CrO₅ is /are
1. One
2. Two
3. Three
4. None of the above

Conversion of PbSO₄ to PbS is:
1. Reduction of S
2. Oxidation of S
3. Dissociation
4. None of the above

10.

Redox reaction among the following is -
1. NaCl + KNO₃ $\to$ NaNO₃ + KCl
2. CaC₂O₄ + 2HCl $\to$ CaCl₂ + H₂C₂O₄
3. Mg(OH)₂ + 2NH₄Cl $\to$ MgCl₂ + 2NH₄OH
4. Zn + 2AgCN $\to$ 2Ag + Zn(CN)₂

11.

The oxidation number of Fe in K₃[Fe(CN)₆] is-
1. +2
2. +3
3. +4
4. +1

12.

It is found that v forms a double salt isomorphous with Mohr's salt. The oxidation number of V in this compound is:
1. +3
2. +2
3. +4
4. -4

13.

The correct order of reducing power of halide ions is:
1. Cl^- > Br^- > I^- > F^-
2. Cl^- > I^- > Br^- > F^-
3. Br^-> Cl^- > I^- > F^-
4. I^- > Br^-> Cl^- > F^-

14.

The reaction during which nitrogen gets oxidised is-
1. ${NH}_{4}^{+}$ $\to$ N₂
2. ${NO}_{3}^{-} \to$ NO
3. NO₂ $\to$ ${NO}_{2}^{-}$
4. ${NO}_{3}^{-}$ $\to$ N $H_{4}^{+}$

15.

Reaction that shows hydrogen as an oxidising agent is:
1. With iodine to give hydrogen iodide
2. With lithium to give lithium hydride
3. With nitrogen to give ammonia
4. With sulphur to give hydrogen sulphide

16.

Fluorine is a strong oxidising agent because:
1. it has several isotopes
2. it is very small and has 7 electrons in valency shell
3. its valency is one
4. it is the first member of the halogen series

17.

The oxidation state of Ni in Ni(CO)₄ is:
1. zero
2. +4
3. +8
4. +2

18.

Sulphurous acid can be used as:
1. Oxidising agent
2. Reducing agent
3. Bleaching agent
4. All of the above

19.

When SO₂ is passed through acidified solution of potassium dichromate, then chromium sulphate is formed. The change in oxidation number of chromium is:
1. +4 to+2
2. +5 to+3
3. +6 to+3
4. +7 to+2

20.

In the reaction;
2Ag + 2H₂SO₄ $\to$ Ag₂SO₄ + 2H₂O + SO₂, H₂SO₄ acts as:
1. Oxidizing agent
2. Reducing agent
3. Dehydrating agent
4. None of the above

21.

Which of the following shows the highest oxidation number in the combined state?
1. Os
2. Ru
3. Xe
4. All of the above

22.

In the preparation of chlorine from HCl; MnO₂ acts as:
1. Reducing agent
2. Oxidising agent
3. Catalytic agent
4. Dehydrating agent

23.

In the equation,
N $O_{2}^{-}$ + H₂O $\to$ N $O_{3}^{-}$ + 2H⁺ + ne^-
n represents
1. 5
2. 1
3. 2
4. 3

24.

Reaction between acidified K₂Cr₂O₇ and iron (II) ions shown by the equation:
Cr₂ $O_{7}^{2 -}$ (aq) + 6Fe²⁺(aq) +14H⁺(aq) $\to$ 2Cr³⁺(aq) + 7H₂O(l) + 6Fe³⁺(aq)
The correct statement among the following is -
1. Colour of the solution changes from green to blue
2. Iron (II) ions are reduced
3. Dichromate ions are reduced
4. Hydrogen ions are reduced

25.

Which metal exhibits more than one oxidation states?
1. Na
2. Mg
3. Al
4. Fe

26.

Among the following, In which iron has the lowest oxidation state?
1. Fe(CO)₅
2. Fe₂O
3. K₄Fe(CN)₆
4. FeSO₄.(NH₄)₂SO₄.6H₂O

27.

When an acidified solution of ferrous ammonium sulphate is treated with KMnO₄ solution, the ion that gets oxidised is:
1. Fe²⁺
2. S $O_{4}^{2 -}$
3. N $H_{4}^{+}$
4. Mn $O_{4}^{-}$

28.

2Na₂S₂O₃+ I₂ $\to$ Na₂S₄O₆ + 2NaI,
the oxidation state of sulphur in tha above reaction:
1. Decreases
2. Increases
3. Remain unchanged
4. None of the above

29.

In a redox change, the oxidant K₂Cr₂O₇is always reduced to:
1. Cr⁵⁺
2. Cr⁴⁺
3. Cr³⁺
4. Cr²⁺

30.

Which of the following reactions does not represent a redox change?
1. CaCO₃ $\to$ CaO + CO₂
2. 2H₂ + O₂ $\to$ 2H₂O
3. Na + H₂O $\to$ NaOH + $\frac{1}{2}$H₂
4. MnCl₃ $\to$ MnCl₂ + $\frac{1}{2}$Cl₂

31.

In the reaction;
3Br₂ + 6C $O_{3}^{2 -}$ + 3H₂O $\to$ 5Br^- + Br $O_{3}^{-}$ + 6HC $O_{3}^{-}$
which statement is correct?
1. Br₂ is oxidised
2. Br₂ is reduced
3. Br₂ is neither oxidised nor reduced
4. Br₂ is oxidised and reduced as well

32.

Amongst the following species that have an atom in (+6) oxidation state is-
1. Mn $O_{4}^{-}$
2. Cr $(CN)_{6}^{3 -}$
3. Ni $F_{6}^{2 -}$
4. CrO₂Cl₂

33.

A metallic oxide contains 20% oxygen. The equivalent weight of metal is
1. 12
2. 16
3. 32
4. 64

34.

Which one is correct about CH₂ = CCl₂?
1. Both carbons are in +2 oxidation state.
2. Both carbons are in +1 oxidation state.
3. One carbon has +2 and other -2 oxidation states.
4. The average oxidation number of carbon is +1.

35.

What is the equivalent weight of H₃PO₃ in the following disproportionation reaction:-
H₃PO₃ $\to$ H₃PO₄ + PH₃
1. $\frac{M}{6}$
2. $\frac{M}{2}$
3. $\frac{2 M}{3}$
4. $\frac{M}{3}$

36.

25.0 g of FeSO₄.7H₂O was dissolved in water containing dilute H₂SO₄, and the volume was made up to 1.0 L. 25.0 mL of this solution required 20 mL of an N/10 KMnO₄ solution for complete oxidation. The percentage of FeSO₄^. 7H₂O in the acid solution is
(1) 78%
(2) 98%
(3) 89%
(4) 79%

37.

Which one of the following orders correctly represents the increasing acid strengths of the given acids?
(1) HOCl <HOClO <HOClO₂< HOClO₃
(2) HOClO <HOCl <HOClO₃<HOClO₂
(3) HOClO₂<HOClO₃<HOClO <HOCl
(4) HOClO₃> HOClO₂<HOClO <HOCl

38.

The valency of Cr in the complex [Cr(H₂O)₄Cl₂]⁺ [MP PMT 2000]
(1) 1
(2) 3
(3) 5
(4) 6

39.

Oxidation number of cobalt in K[Co(CO)₄] is
(1) + 1
(2) + 3
(3) – 1
(4) – 3

40.

The oxidation number of phosphorus in Ba(H₂PO₂)₂ is :
1. – 1
2. + 1
3. + 2
4. + 3

41.

When KMnO₄ acts as an oxidizing agent and ultimately forms $\left[\mathrm{MnO}_4\right]^{-2}, \mathrm{MnO}_2, \mathrm{Mn}_2 \mathrm{O}_3, \mathrm{Mn}^{+2}$
then the number of electrons transferred in each case, respectively, are:

1.	4, 3, 1, 5	2.	1, 5, 3, 7
3.	1, 3, 4, 5	4.	3, 5, 7, 1

42.

For the redox reaction $M n O_{4}^{-} + C_{2} O_{4}^{- 2} + H^{+} \to M n^{2 +} + C O_{2} + H_{2} O$ the correct coefficients of the reactants for the balanced reaction are

	$M n O_{4}^{-}$	$C_{2} O_{4}^{2 -}$	$H^{+}$
(1)	2	5	16
(2)	16	5	2
(3)	5	16	2
(4)	2	16	5

43.

Which of the following is the strongest oxidising agent?
1. $B r O_{3}^{-} / B r^{2 +}, E^{o} = + 1 .50$
2. $F e^{3 +} / F e^{2 +}, E^{o} = + 0 .76$
3. $M n O_{4}^{-} / M n^{2 +}, E^{o} = + 1 .52$
4. $C r_{2} O_{7}^{2 -} / C r^{3 +}, E^{o} = + 1 .33$

44.

Oxidation number of oxygen in potassium super oxide (KO₂) is:
1. – 2
2. – 1
3. – 1/2
4. – 1/4

45.

In a balanced equation $H_{2} S O_{4} + x H I \to H_{2} S + y I_{2} + z H_{2} O$ , the values of x, y, z are :

1.	x = 3, y = 5, z = 2
2.	x = 4, y = 8, z = 5
3.	x = 8, y = 4, z = 4
4.	x = 5, y = 3, z = 4

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