Chemistry - Redox Reactions - Quiz-1

Which of the following is redox reaction ?

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$H_{2} {SO}_{4}$ with NaOH
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Formation of $O_{3}$ in the atmosphere.
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Evaporation of $H_{2} O$
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Oxides of nitrogen form nitrogen & oxygen from lightning

Which of the following is a redox reaction ?

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$2 Na [Ag {(CN)}_{2}] + Zn \to {Na}_{2} [Zn {(CN)}_{4}] + 2 Ag$
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${BaO}_{2} + H_{2} {SO}_{4} \to {BaSO}_{4} + H_{2} O_{2}$
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$N_{2} O_{5} + H_{2} O \to 2 {HNO}_{3}$
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${AgNO}_{3} + KI \to AgI + {KNO}_{3}$

5mL of NHCl, 20 mL of N/2 H₂SO₄ and 30mL of N/3 HNO₃ are mixed together and volume made one litre. The normality of the resulting solution is:

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N/5
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N/10
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N/20
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N/40

When a metal is burnt, its mass is increased by 24 percent. The equivalent mass of the metal will be:

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25
0%

24
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33.3
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76

1g of pure calcium carbonate was found to require 50 mL of dilute HCl for complete reactions. The strength of the HCl solution is given by:

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4N
0%

2N
0%

0.4N
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0.2N

The equivalent mass of H₃PO₄ in the following reaction is,

H₃PO₄+ Ca(OH)₂ $\to$ CaHPO₄ + 2H₂O

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98
0%

49
0%

32.66
0%

40

1.520g of the hydroxide of a metal on ignition gave 0.995 g of oxide. The equivalent mass of metal is:

0%

1.520
0%

0.995
0%

19.00
0%

9.00

0.5 g of fuming H₂SO₄ (oleum) is diluted with water. This solution is completely neutralised by 26.7 mL of 0.4 N NaOH. The percentage of free SO₃ in the sample is:

0%

30.6%
0%

40.6%
0%

20.6%
0%

50%

One g of a mixture of Na₂CO₃ and NaHCO₃ consumes y equivalent of HCl for complete neutralisation. One g of the mixture is strongly heated, then cooled and the residue treated with HCl. How many equivalent of HCl would be required for complete neutralisation?

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2y equivalent
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y equivalent
0%

3y/4 equivalent
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3y/2 equivalent

The chloride of a metal contains 71% chlorine by mass and the vapour density of it is 50. The atomic mass of the metal will be:

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29
0%

58
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35.5
0%

71

The equivalent mass of Zn(OH)₂ in the following reaction is equal to its,

Zn(OH)₂ + HNO₃ $\to$ Zn(OH)(NO₃) + H₂O :

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Formula mass/1
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Formula mass/2
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2 x formula mass
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3 x formula mass

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?

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0.4 N
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0.5 N
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1.05 N
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0.15 N

0.7 g of Na₂CO₃.xH₂O were dissolved in water and the volume was made to 100mL, 20mL of this solution required 19.8 mL of N/10 HCl for complete neutralization. The value of x is:

0%

7
0%

3
0%

2
0%

5

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:

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the atomic mass of the metal is 8
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the atomic mass of the metal is 4
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the equivalent mass of the metal is 4
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the equivalent mass of the metal is 8

An oxide of metal has 20% oxygen, the equivalent mass of oxide is:

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32
0%

40
0%

48
0%

52

How much water is to be added to dilute 10 mL of 10N HCl to make it decinormal?

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990mL
0%

1010 mL
0%

100mL
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1000mL

W₁ g of an element combines with oxygen forming W₂ g of its oxide. The equivalent mass of the element is:

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[W₁ / W₂]x8
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[W₁ / W₂-W₁]x8
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[W₂-W₁/W₁ ]x8
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[W₁ / W₁-W₂]x8

The normality of 4% (mass/Vol.) NaOH is:

0%

0.1
0%

1.0
0%

0.05
0%

0.01

The number of peroxide linkages in CrO₅ is /are

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One
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Two
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Three
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None of the above

Conversion of PbSO₄ to Pbs is:

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Reduction of S
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Oxidation of S
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Dissociation
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None of the above

An aqueous solution of SO₂ reacts with H₂S to precipitate sulfur. Here SO₂ acts as:

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Catalyst
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Reducing agent
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Oxidising agent
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Acid

Redox reaction among the following is -

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NaCl + KNO₃ $\to$ NaNO₃ + KCl
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CaC₂O₄ + 2HCl $\to$ CaCl₂ + H₂C₂O₄
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Mg(OH)₂ + 2NH₄Cl $\to$ MgCl₂ + 2NH₄OH
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Zn + 2AgCN $\to$ 2Ag + Zn(CN)₂

Reaction that represents reduction of hydrogen is -

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Carbon Monoxide + Copper Oxide $\to$ Carbon Dioxide + Copper
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Copper Oxide + Hydrochlorid Acid $\to$ Water + Copper Chloride
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Steam + Iron $\to$ Hydrogen + Iron oxide
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Hydrogen+ Iron Oxide $\to$ Water + Iron

The oxidation number of Fe in K₃[Fe(CN)₆] is-

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+2
0%

+3
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+4
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+1

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

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+3
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+2
0%

+4
0%

-4

The correct order of reducing power of halide ions is:

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Cl^- > Br^- > I^- > F^-
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Cl^- > I^- > Br^- > F^-
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Br^-> Cl^- > I^- > F^-
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I^- > Br^-> Cl^- > F^-

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

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0 to +2
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+2 to +4
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+4 to +2
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+4 to +6

The reaction during which nitrogen gets oxidised is-

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${NH}_{4}^{+}$ $\to$ N₂
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${NO}_{3}^{-} \to$ NO
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NO₂ $\to$ ${NO}_{2}^{-}$
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${NO}_{3}^{-}$ $\to$ N $H_{4}^{+}$

Reaction that shows hydrogen as an oxidising agent is -

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With ioding to give hydrogen iodide
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With lithium to give lithium hydride
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With nitrogen to give ammonia
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With sulphur to give hydrogen sulphide

Fluorine is a strong oxidising agent because:

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it has several isotopes
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it is very small and has 7 electrons in valency shell
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its valency is one
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it is the first member of the halogen series

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Practice Chemistry Quiz Questions and Answers

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Practice Chemistry Quiz Questions and Answers

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