Test: Mole Concept, Volumetric & Redox - 1

Question 1

4.4g of CO₂ and 2.24 litre of H₂at STP (273.15 K and 1 atm pressure) are mixed in a container. The total of molecules present in the container will be

Accepted Answer

12.044 x 10²²

Answer

6.023 x 10²³

Answer

6.023 x 10²²

Answer

6.023 x 10²⁴

Question 2

4I^– + Hg²⁺ → HgI₄^2– ; 1 mole of each Hg²⁺ and I^– will form:

Accepted Answer

0.25 mole of HgI₄^2–

Answer

1 mole of HgI₄^2–

Answer

0.5 mole of HgI₄^2–

Answer

2 mole of HgI₄^2–

Question 3

How many grams of I₂ are present in a solution which requires 40 ml of 0.11N Na₂S₂O₃ to react with it via the reaction:
S₂O₃^2– + I₂ → S₄O₆^2– + 2I^–?

Accepted Answer

0.558g

Answer

12.7g

Answer

25.4g

Answer

11.4g

Question 4

Two elements A (atomic mass = 75) and B (atomic mass = 16) combine to yield a compound. The % by weight of A in the compound was found to be 75.08. The formula of compound is:

Accepted Answer

A2B3

Answer

A2B

Answer

AB

Answer

AB2

Question 5

What weight of HNO₃ is needed to convert 5g of Iodine into Iodic acid according to the reaction:
I₂ + HNO₃→ HIO₃ + NO₂ +H₂O

Accepted Answer

12.4g

Answer

24.8g

Answer

0.248g

Answer

49.6g

Question 6

In the reaction, VO + Fe₂O₃ → FeO + V₂O₅, the equilvalent weight of V₂O₅ is equal to its

Accepted Answer

Mol. Wt./6

Answer

Mol. Wt.

Answer

Mol. Wt./4

Answer

Mol. Wt./8

Question 7

When BrO₃^– ion reacts with Br^– ion in acid solution Br₂ is liberated. The eq. weight of KBrO₃ in this reaction is:

10e + 2Br⁵⁺→ Br0₂

Accepted Answer

M/5

Answer

M/8

Answer

M/3

Answer

M/6

Question 8

The hydrated salt, Na₂SO₄.nH₂O, undergoes 55.9 % loss in weight on heating and become anhydrous. The value of n will be:

Accepted Answer

10

Answer

5

Answer

3

Answer

7

Question 9

When a metal is burnt, its weight is increased by 24%. The eq. weight of the metal will be:

Accepted Answer

33.3

Answer

25

Answer

24

Answer

76

Question 10

One mole of potassium chlorate is thermally decomposed and excess of aluminum is burnt in the gaseous product .How many moles of aluminum oxide are formed?

Accepted Answer

1

Answer

1.5

Answer

2

Answer

3

Question 11

How much Cl₂ at STP is liberated when one mole of KMnO₄ reacts with HCl ?

Accepted Answer

56 L

Answer

11.2 L

Answer

22.4 L

Answer

44.8 L

Question 12

Minimum quantity of H₂S needed to precipitate 63.5g of Cu²⁺ is nearly:

Accepted Answer

34g

Answer

63.5 g

Answer

20g

Answer

126g

Question 13

2g of CaCO₃ was treated with 0.1M HCl (500 ml). The volume of CO₂ evolved at STP after heating the solution is:

Accepted Answer

0.448 L

Answer

0.224 L

Answer

4.48 L

Answer

44.8 L&#160;

Question 14

10g of limestone on heating produces 4.2g of CaO. the percentage purity of CaCO3 in limestone is:

Accepted Answer

75 %

Answer

50%

Answer

72%

Answer

100%

Question 15

‘x’ g of KClO₃ on decomposition gives ‘y’ ml of O₂ at STP. The % purity of KClO₃ would be

Accepted Answer

Answer

Answer

Answer

Question 16

33.6g of an impure sample of sodium bicarbonate when heated strongly gave 4.4g of CO₂. The % purity of NaHCO₃ would be:

Accepted Answer

50%

Answer

25%

Answer

75%

Answer

100%

Question 17

0.16g of dibasic acid required 25ml of N/10 NaOH for complete neutralization. Molecular wt. of acid is:

Accepted Answer

128

Answer

32

Answer

64

Answer

256

Question 18

The molar coefficients of AsO₃^3– and MnO₄^- in the reaction are:

AsO₃^3– + MnO₄^Θ → AsO₄^3– + MnO₂

Accepted Answer

3, 2

Answer

2, 3

Answer

2, 2

Answer

3, 3

Question 19

Which of the following is a disproportionation reaction?

Accepted Answer

Cu₂O + 2H⁺ → Cu + Cu²⁺ + H₂O

Answer

CaCO₃ + 2H⁺ → Ca²⁺ + H₂O + CO₂

Answer

2CrO₄^2– + 2H⁺ → Cr₂O₇^2– + H₂O

Answer

Cr₂O₇^2– + 2OH^– → 2CrO₄^2– +H₂O

Question 20

Hydrogen and oxygen combine to form H₂O₂ and H₂O containing 5.93% and 11.2 % hydrogen respectively. The data illustrates:

Accepted Answer

Law of multiple proportion

Answer

Law of conservation of mass

Answer

Law of constant proportion

Answer

Law of reciprocal proportion

Mole Concept, Volumetric & Redox - 1 - Free MCQ Practice Test with solutions,

MCQ Practice Test & Solutions: Test: Mole Concept, Volumetric & Redox - 1 (20 Questions)

4.4g of CO₂ and 2.24 litre of H₂at STP (273.15 K and 1 atm pressure) are mixed in a container. The total of molecules present in the container will be

4I^– + Hg²⁺ → HgI₄^2– ; 1 mole of each Hg²⁺ and I^– will form:

How many grams of I₂ are present in a solution which requires 40 ml of 0.11N Na₂S₂O₃ to react with it via the reaction:
S₂O₃^2– + I₂ → S₄O₆^2– + 2I^–?

Two elements A (atomic mass = 75) and B (atomic mass = 16) combine to yield a compound. The % by weight of A in the compound was found to be 75.08. The formula of compound is:

What weight of HNO₃ is needed to convert 5g of Iodine into Iodic acid according to the reaction:
I₂ + HNO₃→ HIO₃ + NO₂ +H₂O

In the reaction, VO + Fe₂O₃ → FeO + V₂O₅, the equilvalent weight of V₂O₅ is equal to its

When BrO₃^– ion reacts with Br^– ion in acid solution Br₂ is liberated. The eq. weight of KBrO₃ in this reaction is:
10e + 2Br⁵⁺→ Br0₂

The hydrated salt, Na₂SO₄.nH₂O, undergoes 55.9 % loss in weight on heating and become anhydrous. The value of n will be:

When a metal is burnt, its weight is increased by 24%. The eq. weight of the metal will be:

One mole of potassium chlorate is thermally decomposed and excess of aluminum is burnt in the gaseous product .How many moles of aluminum oxide are formed?

How much Cl₂ at STP is liberated when one mole of KMnO₄ reacts with HCl ?

Minimum quantity of H₂S needed to precipitate 63.5g of Cu²⁺ is nearly:

2g of CaCO₃ was treated with 0.1M HCl (500 ml). The volume of CO₂ evolved at STP after heating the solution is:

10g of limestone on heating produces 4.2g of CaO. the percentage purity of CaCO3 in limestone is:

‘x’ g of KClO₃ on decomposition gives ‘y’ ml of O₂ at STP. The % purity of KClO₃ would be

33.6g of an impure sample of sodium bicarbonate when heated strongly gave 4.4g of CO₂. The % purity of NaHCO₃ would be:

0.16g of dibasic acid required 25ml of N/10 NaOH for complete neutralization. Molecular wt. of acid is:

The molar coefficients of AsO₃^3– and MnO₄^- in the reaction are:
AsO₃^3– + MnO₄^Θ → AsO₄^3– + MnO₂

Which of the following is a disproportionation reaction?

Hydrogen and oxygen combine to form H₂O₂ and H₂O containing 5.93% and 11.2 % hydrogen respectively. The data illustrates:

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Mole Concept, Volumetric & Redox - 1 - Free MCQ Practice Test with solutions,

MCQ Practice Test & Solutions: Test: Mole Concept, Volumetric & Redox - 1 (20 Questions)

4.4g of CO2 and 2.24 litre of H2 at STP (273.15 K and 1 atm pressure) are mixed in a container. The total of molecules present in the container will be

4I– + Hg2+ → HgI42– ; 1 mole of each Hg2+ and I– will form:

How many grams of I2 are present in a solution which requires 40 ml of 0.11N Na2S2O3 to react with it via the reaction: S2O32– + I2 → S4O62– + 2I–?

Two elements A (atomic mass = 75) and B (atomic mass = 16) combine to yield a compound. The % by weight of A in the compound was found to be 75.08. The formula of compound is:

What weight of HNO3 is needed to convert 5g of Iodine into Iodic acid according to the reaction: I2 + HNO3→ HIO3 + NO2 +H2O

In the reaction, VO + Fe2O3 → FeO + V2O5, the equilvalent weight of V2O5 is equal to its

When BrO3– ion reacts with Br– ion in acid solution Br2 is liberated. The eq. weight of KBrO3 in this reaction is:10e + 2Br5+ → Br02

The hydrated salt, Na2SO4.nH2O, undergoes 55.9 % loss in weight on heating and become anhydrous. The value of n will be:

When a metal is burnt, its weight is increased by 24%. The eq. weight of the metal will be:

One mole of potassium chlorate is thermally decomposed and excess of aluminum is burnt in the gaseous product .How many moles of aluminum oxide are formed?

How much Cl2 at STP is liberated when one mole of KMnO4 reacts with HCl ?

Minimum quantity of H2S needed to precipitate 63.5g of Cu2+ is nearly:

2g of CaCO3 was treated with 0.1M HCl (500 ml). The volume of CO2 evolved at STP after heating the solution is:

10g of limestone on heating produces 4.2g of CaO. the percentage purity of CaCO3 in limestone is:

‘x’ g of KClO3 on decomposition gives ‘y’ ml of O2 at STP. The % purity of KClO3 would be

33.6g of an impure sample of sodium bicarbonate when heated strongly gave 4.4g of CO2. The % purity of NaHCO3 would be:

0.16g of dibasic acid required 25ml of N/10 NaOH for complete neutralization. Molecular wt. of acid is:

The molar coefficients of AsO33– and MnO4- in the reaction are:AsO33– + MnO4Θ → AsO43– + MnO2

Which of the following is a disproportionation reaction?

Hydrogen and oxygen combine to form H2O2 and H2O containing 5.93% and 11.2 % hydrogen respectively. The data illustrates:​

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4.4g of CO₂ and 2.24 litre of H₂at STP (273.15 K and 1 atm pressure) are mixed in a container. The total of molecules present in the container will be

4I^– + Hg²⁺ → HgI₄^2– ; 1 mole of each Hg²⁺ and I^– will form:

How many grams of I₂ are present in a solution which requires 40 ml of 0.11N Na₂S₂O₃ to react with it via the reaction:
S₂O₃^2– + I₂ → S₄O₆^2– + 2I^–?

What weight of HNO₃ is needed to convert 5g of Iodine into Iodic acid according to the reaction:
I₂ + HNO₃→ HIO₃ + NO₂ +H₂O

In the reaction, VO + Fe₂O₃ → FeO + V₂O₅, the equilvalent weight of V₂O₅ is equal to its

When BrO₃^– ion reacts with Br^– ion in acid solution Br₂ is liberated. The eq. weight of KBrO₃ in this reaction is:
10e + 2Br⁵⁺→ Br0₂

The hydrated salt, Na₂SO₄.nH₂O, undergoes 55.9 % loss in weight on heating and become anhydrous. The value of n will be:

How much Cl₂ at STP is liberated when one mole of KMnO₄ reacts with HCl ?

Minimum quantity of H₂S needed to precipitate 63.5g of Cu²⁺ is nearly:

2g of CaCO₃ was treated with 0.1M HCl (500 ml). The volume of CO₂ evolved at STP after heating the solution is:

‘x’ g of KClO₃ on decomposition gives ‘y’ ml of O₂ at STP. The % purity of KClO₃ would be

33.6g of an impure sample of sodium bicarbonate when heated strongly gave 4.4g of CO₂. The % purity of NaHCO₃ would be:

The molar coefficients of AsO₃^3– and MnO₄^- in the reaction are:
AsO₃^3– + MnO₄^Θ → AsO₄^3– + MnO₂

Hydrogen and oxygen combine to form H₂O₂ and H₂O containing 5.93% and 11.2 % hydrogen respectively. The data illustrates: