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# Frank Modern Certificate Solution for Class 10 Chemistry Chapter 5 - Mole Concept And Stoichiometry

## Frank Textbook Solutions Chapter 5 - Mole Concept And Stoichiometry

Frank Textbook Solutions are considered extremely helpful for solving difficult questions in the ICSE Class 10 Chemistry exam. TopperLearning Textbook Solutions are compiled by our subject experts. Herein, you can find all the answers to the questions of   Chapter 5 - Mole Concept And Stoichiometry for the Frank textbook.

Frank Textbook Solutions for class 10 are in accordance with the latest ICSE syllabus, and they are amended from time to time to be most relevant. Our free Frank Textbook Solutions for ICSE Class 10 Chemistry will give you deeper insight on the chapters and will help you to score more marks in the final examination. ICSE Class 10 students can refer to our solutions while doing their homework and while preparing for the exam.

Exercise/Page

## Frank Modern Certificate Solution for Class 10 Chemistry Chapter 5 - Mole Concept And Stoichiometry Page/Excercise 115

Solution 14

Solution 1

(a) Gay-Lussac's law: It states that 'when gases react, they do so in volumes which bear a simple ratio to one another, and also to the volume of the gaseous product, provided all the volumes are measured at the same temperature and pressure'.
(b) Avogadro's law : It states that 'Under the same conditions of temperature and pressure, equal volumes of all gases contain the same number of molecules'.

Solution 2

Solution 3

When stating the volume of a gas, the pressure and temperature should also be given because the volume of a gas is highly susceptible to slight change in pressure and temperature of the gas.

Solution 4

Solution 5

Solution 6

Solution 7

(a) Gram atom: "The quantity of the element which weighs equal to its gram atomic mass is called one gram atom of that element".
For example: The gram atomic mass of hydrogen is 1g. So, 1g of hydrogen is 1 gram atom of hydrogen.
(b) Gram mole: "A sample of substance with its mass equal to its gram molecular mass is called one gram molecule of this substance or one gram mole".
For example: Gram molecular mass of oxygen is 32 g. So One gram mole of oxygen is 32g.

Solution 8

Solution 9

Empirical formula:"Empirical formula of a compound is the formula which gives the number of atoms of different elements present in one molecule of the compound, in the simplest numerical ratio".
Molecular formula: "Molecular formula of a compound denotes the actual number of atoms of different elements present in one molecule of the compound".

Solution 10

(a) The empirical formula of C6H6 is: CH
(b) The empirical formula of C6H12O6 is: CH2O.
(c) The empirical formula of C2H2 is: CH
(d) The empirical formula of CH3COOH is: CH2O.

Solution 11

Three pieces of information conveyed by the formula H2O is that:

It shows that there are 2hydrogen atoms and 1oxygen atoms present in H2O.
The hydrogen and oxygen atoms are present in simplest whole number ratio of 2:1.
It represents one molecule of compound water.

Solution 12

Solution 13

Solution 15

(a) Na2SO4.10H2O.
(b) C6H12O6.

Solution 16

Solution 17

Solution 18

Solution 19

Solution 20

Solution 21

Solution 22

Solution 23

Solution 24

Solution 25

Solution 26

Solution 27

Solution 28

Solution 29

Solution 30

Solution 31

Solution 1996-1

Solution 1996-2

Solution 1996-3

Solution 1996-4

Solution 1997-1

Solution 1997-2

Solution 1997-3

Solution 1997-4

Solution 1998-1

Solution 1998-2

Solution 1999-1

Solution 1999-2

Solution 1999-3

Solution 2000-1

Solution 2000-2

## Frank Modern Certificate Solution for Class 10 Chemistry Chapter 5 - Mole Concept And Stoichiometry Page/Excercise 119

Solution 2001-1

Gay - Lussac proposed this law.

Solution 2001-2

Molecular mass of ethane = 30
According to Gay-Lussac's law:
2 vol. of C2H6 requires= 7 vol. of oxygen
Vol. of C2H6 = 2 vol. = 100 L
Vol. of oxygen required = 7 vol. =350 L

Solution 2001-3

Solution 2001-4

The term is vapour density.

Solution 2001-5

Solution 2001-6

Solution 2001-7

Solution 2002-1

Solution 2002-2

Solution 2002-3

Solution 2003-1

Solution 2004-1

Solution 2004-2

Solution 2005-1

Solution 2006-1

Solution 2006-2

Solution 2006-3

Solution 2006-4

Solution 2007-1

## Frank Modern Certificate Solution for Class 10 Chemistry Chapter 5 - Mole Concept And Stoichiometry Page/Excercise 122

Solution 2007-2

Solution 2008-1

The gas laws which relates the volume of a gas to the number of molecules of the gas is avogadro's law

Solution 2008-2

Solution 2008-3

## Frank Modern Certificate Solution for Class 10 Chemistry Chapter 5 - Mole Concept And Stoichiometry Page/Excercise 123

Solution 2009-1

The relative molecular mass of the gas is 10.

Solution 2009-2

Solution 2009-3

The correct statement is that equal volumes of all gases under identical conditions contain the same number of molecules.

Solution 2009-4

Solution 2010-1

(ii) Molecular mass of NH4(NO3) = 80

H = 1, N = 14, O = 16

% of nitrogen

As 80 g of NH4 (NO3) contains 28 g of nitrogen,

% of nitrogen

As80 g of NH4(NO3) contains48 g of oxygen

Solution 2010-2

(i) Equation for the reaction of calcium carbonate with dilute hydrochloric acid:

(ii) Relative molecular mass of calcium carbonate=100

Mass of 4.5 moles of calcium carbonate

= No. of moles× Relative molecular mass

= 4.5×100

= 450g

(iii)

As100g of calcium carbonate gives 22.4dm3 of CO2,

(iv) Molecular mass of calcium carbonate =100

Relative molecular mass of calcium chloride =111

As 100 g of calcium carbonate gives 111g of calcium chloride,

(v) Molecular mass of HCl=36.5

Molecular mass of calcium carbonate =100

As 100 g of calcium carbonate gives (2×36.5)= 73g of HCl,

## Frank Modern Certificate Solution for Class 10 Chemistry Chapter 5 - Mole Concept And Stoichiometry Page/Excercise 124

Solution 2011-1

(i) Atomic mass: S = 32 and O = 16

Molecular mass of SO2=32+(2×16)=64g

As 64 g of SO2 = 22.4dm3,

(ii) Gay-Lussac's law: When gases react, they do so in volumes which bear a simple ratio to one another and to the volume of the gaseous product, if all the volumes are measured at the same temperature and pressure.

(iii) C3H8 + 5O2  3CO2 + 4H2O

Molar mass of propane = 44

44 g of propane requires 5 × 22.4 litres of oxygen at STP.

Solution 2011-2

 Element Relative atomic mass % Compound Atomic ratio Simplest ratio H 1 2.13 2.13/1 = 2.13 2 C 12 12.67 12.67/12 = 1.055 2 Br 80 85.11 85.11/80 = 1 1

Empirical formula = CH2Br

n(Empirical formula mass of CH2Br) = Molecular mass (2 × VD)

n(12 + 2 + 80) = 94 × 2

n = 2

Molecular formula = Empirical formula × 2

= (CH2Br) × 2

= C2H4Br2

Solution 2011-3

(i) 1022 atoms of sulphur

6.022 × 1023 atoms of sulphur will have mass = 32 g

(ii) 0.1 mole of carbon dioxide

1 mole of carbon dioxide will have mass = 44 g

0.1 mole of carbon dioxide will have mass = 4.4 g

Solution 2013-1

Solution 2013-2

Solution 2014-1

## Frank Modern Certificate Solution for Class 10 Chemistry Chapter 5 - Mole Concept And Stoichiometry Page/Excercise 125

Solution 2014-2

(i) Vapour density

(ii) Ionisation

Solution 2014-3

(i) Avogadro's law:Equal volumes of all gases under similar conditions of temperature and pressure contain the same number of molecules.

(ii)

Solution 2015-1

6.02 × 1023 atoms of carbon

Solution 2015-2

(i) 3.2 g of S has number of atoms = 6.023 × 1023 x 3.2 /32

= 0.6023 × 1023

So, 0.6023 × 1023 atoms of Ca has mass=40 × 0.6023 ×1023/6.023 × 1023 = 4g

(ii) 6 litres of hydrogen and 4 litres of chlorine when mixed result in the formation of 8 litres of HCl gas.

When water is added to it, it results in the formation of hydrochloric acid. Chlorine acts as a limiting agent leaving behind only 2 litres of hydrogen gas.

Therefore, the volume of the residual gas will be 2 litres.

(iii)

Solution 2015-3

(i)

(ii) 252 g of ammonium dichromate gives 22.4 dm3of N2

(iii)

(iv) 252 g of ammonium dichromate gives 152 g of CrO3

Solution 2016-1

Solution 2016-2

% of carbon = 82.76%

% of hydrogen = 100 - 82.76 = 17.24%

 Element % Weight Atomic Weight Relative No. of moles Simplest Ratio C 82.76 12 82.76/12 = 6.89 6.89/6.8 = 1 × 2 = 2 H 17.24 1 17.24/1 = 17.24 17.24/6.89 = 2.5 × 2 = 5

Empirical formula = C2H5

Empirical formula weight = 2 × 12 + 1 × 5 = 24 + 5 = 29

Vapour density = 29

Relative molecular mass = 29 × 2 = 58

## Frank Modern Certificate Solution for Class 10 Chemistry Chapter 5 - Mole Concept And Stoichiometry Page/Excercise 126

Solution 2016-3

Solution 2016-4

Mass of gas = 32 g

Volume occupied by 32g of gas = 20litres

Solution 2016-5

2Ca(NO3)2 2CaO + 4NO2 + O2

Molecular weight of 2Ca(NO3)2 = 2[40+2(14+48) = 32g

Molecular weight of CaO = 2(40 + 16) = 112g

328 g of Ca(No3]2 liberates 4 moles of NO2

328 g of Ca (NO3)2 liberates 4 × 22.4 L of NO2

Solution 2016-6

Solution 2017-1

(a)

(b)

(c)

Solution 2017-2

(a)

Given:

C3H8 + 5O2 3CO2 + 4H2O

Volume of air = 1000 cm3

Percentage of oxygen in air = 20%

From the given information,

According to Gay-Lussac's law,

1 vol. of propane consumes 5 vol. of oxygen.

Volume of oxygen = 1000 cm3 × 20% = 200 cm3

Therefore,

Volume of propane burnt for every 200 cm3 of oxygen,

40 cm3of propane is burnt.

(b)

(i) Given:

Volume of gas at STP = 11.2 litres

Mass of gas at STP = 24 g

Gram molecular mass = ?

Mass of 22.4 L of a gas at STP is equal to its gram

molecular mass.

11.2 L of the gas at STP weighs 24 g

So,

22.4 L of the gas will weigh

Gram molecular mass = 48 g

Solution 2017-3

(a)

Given:

Mass of hydrogen = 1 kg at 298 K and 1 atm pressure

Moles of hydrogen =?

(b) Molecular mass of CO2 = 12 + 2 × 16 = 44g

So, vapour density (VD) = mol. Mass/2 = 44/2 = 22

(c) According to Avogadro's law, equal volumes of all gases under similar conditions of temperature and pressure contain equal number of molecules.

(d) So, number of molecules of carbon dioxide in the cylinder = number of molecules of hydrogen in the cylinder = X

## Browse Study Material

TopperLearning provides step-by-step solutions for each question in each chapter in the Frank textbook recommended by ICSE schools. Access Chapter 5 - Mole Concept And Stoichiometry here. Our Frank Textbook Solutions for ICSE Class 10  Chemistry are designed by our subject matter experts. These solutions will help you to revise the whole chapter, so you can clear your fundamentals before the examination.

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