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Ncert Solutions For Class 11 Chemistry Chapter 1

Adda247 provides NCERT solutions for class 11 chemistry chapter 1. The NCERT Solutions provided here will enhance the concepts of the students, as well as suggest alternative methods to solve particular problems to the teachers.

These NCERT Solutions Class 11 chemistry chapter 1 are presented in a very simple language so that you can understand the basic of chemistry with ease. These NCERT Solutions class 11 Chemistry cover chapters 1 to 14 with all important questions and answers explained in a detailed way.

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The solutions available are in depth and simplest way. Thus will help the students beyond examination marks. This will help them develop a core understanding of the subject. Because this subject demands to understand rather than just memorizing solutions of Class 11 Chemistry. Here below we are providing you with the overview of all the chemistry Class 11 Chapters that are there in the NCERT textbook.

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Benefits of Solutions of NCERT class 11 Chemistry:

• NCERT Solutions for Class 11 is helpful to solve questions from other reference books too.
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NCERT Solutions for Class 11 Chemistry Chapter 1 – Some Basic Concepts of Chemistry

Chemistry is the science of molecules and their transformations. It is the science not so much of the one hundred elements but of the infinite variety of molecules that may be built from them.

Chemistry is important because everything you do is chemistry! Even your body is made of chemicals. Chemical reactions occur when you breathe, eat, or just sit there reading. All matter is made of chemicals, so the importance of chemistry is that it’s the study of everything.

Adda247 provides you with Class 11 Chemistry NCERT Solutions Chapter 1. Our experts of Chemistry explain the solutions of all questions as per the NCERT pattern. Some basic concepts of Chemistry Class11 NCERT Solutions are given to make your study simplistic and enjoyable at Adda247. You can get NCERT Solutions for Class 11 Chemistry Chapter 1 PDF download from Adda247 website to assist you through the complete syllabus properly and obtain the best marks in your examinations.

The Chapter touches upon topics such as the importance of Chemistry, atomic mass, and molecular mass. Some basic laws and theories in Chemistry such as Dalton’s atomic theory, Avogadro’s law and the law of conservation of mass are also discussed in this chapter.

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NCERT Solutions for Class 11 Chemistry Chapter 1 Subtopics

• Importance of Chemistry.
• Nature of Matter
• Properties of Matter and Their Measurement.
• The International System of Units.
• Mass And Weight
• Uncertainty in Measurement.
• Scientific notation
• Significant Figures
• Dimensional Analysis
• Laws of Chemical Combinations
• Laws of Conservation of Mass
• Law of Definite proportions
• Law of Multiple Proportions
• Gay Lussac’s Law of Gaseous Volumes
• Avogadro Law
• Dalton’s Atomic Theory
• Atomic and Molecular Masses
• Atomic mass
• Average Atomic Mass
• Molecular Mass
• Formula Mass
• Mole concept And Molar Masses
• Percentage Composition
• Empirical Formula for Molecular Formula
• Stoichiometry and Stoichiometry Calculations
• Limiting Reagent
• Reactions In Solutions

 Read Ncert Solutions Class 12  Chemistry

 

Key features of NCERT solutions for class 11 Chemistry chapter 1: Some Basic Concepts of Chemistry

• The NCERT solution provide clear and precise answer.
• The columns are used wherever necessary.

 

 

Important questions of NCERT Solutions of Chemistry Class 11 Chapter 1

Question: 1 Calculate the molar mass of the following:

• H₂O
• CO₂
• CH₄

Answer:

• H₂O

The molecular mass of water

= (2 x atomic mass of hydrogen) + (1 x atomic mass of oxygen)

= [2(1.0084) + 1(16.00u)]

= 2.016 u + 16.00u

= 18.016 u

= 18.02 u

• CO₂

The molecular mass of carbon dioxide

= (1 x atomic mass of carbon) + (2 x atomic mass of oxygen)

= [1(12.011u) + 2(16.00 u)

= 12.011 u + 32.00 u

= 44.01 u

• CH₄

= The molecular mass of methane

= (1 x atomic mass of carbon) + (4 x atomic mass of hydrogen)

= [1(12.011 u ) + 4(1.0084 u)

= 12.011 u + 4.032 u

= 16.043 u

 

Question: 2 Calculate the mass percent of different elements present in sodium sulphate (Na₂SO₄).

Answer:

The molecular formula of the sodium sulphate is Na2SO4

Molar mass of Na2SO4 = [(2 x 23.0) + (32.066) + 4(16.00)]

= 142.066 g

Mass percentage = Mass of that element in the compound x 100 / Molar mass of the compound

:Mass percent of the sodium:

= 46.0g x 100 / 142.066g

= 32.37 g

= 32.4%

: Mass percent of sulphur:

= 32.066 g x 100 / 142.066g

= 22.57

= 22. 6%

Mass percent of oxygen:

= 64.0 g x 2100 / 142.066 g

= 45.049

= 45.05%

 

Question: 3 Determine the empirical formula of an oxide of iron which has 69.9% iron and 30.1% oxygen by mass.

Answer:

% of iron by mass 69.9%

% 0f oxygen by mass 30.1%

Relative moles of iron in iron oxide:

= % of iron by mass / Atomic mass of iron

= 69.9 / 55.85

= 1.25

Relative moles of oxygen in iron oxide:

= % of oxygen by mass / Atomic mass of oxygen

= 30.1 / 16.00

= 1.88

Simplest molar ratio of iron to oxygen:

= 1.25 : 1.88

= 1 : 1.5

= 2 : 3

: The empirical formula of iron oxide is Fe2O3.

 

Question: 4 Calculate the amount of carbon dioxide that could be produced when

• 1 mole of carbon is burnt in air.
• 1 mole of carbon is burnt in 16g of dioxygen.
• 2 moles of carbon are burnt in 16g of dioxygen.

Answer:

The balanced reaction of combustion of carbon can be written as:

C + O₂ à CO₂

• As per the balanced equation, 1 mole of carbon burns in 1 mole of dioxygen to produce 1 mole of carbon dioxide.
• According to the equation, only 16 g dioxygen is available. Hence, it will react with 0.5 mole of carbon to give 22 g of carbon dioxide. Hence, it is a limiting reagent.
• According to the question, only 16 g dioxygen is available. It is a limiting reagent. Thus, 16 g of dioxygen can combine with only 0.5 mole of carbon to give 22 g of carbon dioxide.

 

Question: 5 Calculate the mass of sodium acetate (CH₃COONa) required to make 500mL of 0.375 molar aqueous solution. Molar mass of sodium acetate is 82.0245 g mol^-1.

Answer:

0.375 M aqueous solution of sodium acetate

= 1000 mL of solution containing 0.375 moles of sodium acetate

: Number of moles of sodium acetate in 500 Ml

= 0.375 x 500 / 1000

= 0.1875 mole

Molar mass of sodium acetate = 82.0245 g mole^-1 (given)

: Required mass of sodium acetate = 82.0245 g mole^-1(0.1875 mole)

= 15.38 g

 

Question: 6 Calculate the concentration of nitric acid in moles per litre in a sample which has a density. 1.41 g mol^-1 and the mass percent of nitric acid in it being 69%.

Answer:

Mass percent of nitric acid is the sample = 69%

The 100g 0f nitric acid contains 60 g of nitric acid by mass

Molar mass of nitric acid (HNO3)

= {1 + 14 + 3(16)} gmol^-1

= 1 + 14 + 18

= 63 g mol^-1

: Number of moles in 69 g of HNO3

= 69 g / 63 g mol^-1

= 1.095 mol

Volume of 100g of nitric acid solution

= Mass of solution / density of solution

= 100g / 1.41 gmL^-1

= 70.92 Ml = 70.92 x 10^-3

= 15.44mol/L

Concentration of nitric acid = 15.44 mol/L

 

Question: 7 How much copper can be obtained from 100g of copper sulphate (CuSO₄).

Answer:

1 mole of CuSO₄ contains 1 mole of copper

Molar mass of CuSO₄ = (63.5) + (32.00) + 4(16)

= 159.5 g

159.5 g of CuSO₄ contains 63.5 g of copper

= 100 g of CuSO₄ will contains 63.5 x 100g / 159.5 of copper

= Amount of copper that can be obtained from 100g of CuSO₄ = 63.5 x 100 / 159.5

= 39.81 g

 

Question: 8 Determine the molecular formula of an oxide of iron in which the mass percent of iron and oxygen are 69.9 and 30.1 respectively.

Answer:

From the available data Percentage of iron = 69.9

Percentage of oxygen= 30.1

Total percentage of iron & oxygen= 69.9+30.1= 100%

Step 1 calculation of simplest whole number ratios of the elements

Element	Percentage	Atomic mass	Atomic ratio	Simplest ratio	Simplest whole ratio
F = 1e	69.9	55.84	69.9 / 55.84 = 1.25	1.25	2
O	30.1	16	30.1 / 16 = 1.88	1.88 = 1.5	3

 

Step 2  Writing the empirical formula of the compound

The empirical formula of the compound = Fe2 O3

Step 3 determination of molecular formula of the compound

Empirical formula mass = 2 X69.9 + 3 X16=187.8 amu

Molecular mass of oxide= 159.69g/mol(given)

Now we know molecular formula = n x Empirical formula

And n= molecular mass / empirical formula mass= 159.69/187.8 = 0.85 = approx 1

Therefore molecular formula = n x empirical formula

=1 x(Fe2O3) = Fe2O3

The molecular formula of the oxide is Fe2O3

 

Question: 9 Calculate the atomic mass (average) of chlorine using the following data:

                                       % Natural abundance            Molar Mass

³⁵Cl                                              75.77                                  34.9689

³⁷Cl                                              24.23                                  36.9659

Answer:

The average atomic mass of chlorine

= (Fractional abundance of ³⁵Cl) + (Molar mass of ³⁶Cl) + (Fractional abundance of ³⁷Cl)

= [{75.77 / 100}(34.9689 u)} + {(24.23 / 100)(36.9659)}[]

= 35.4527 u.

 

Question: 10 In three moles of ethane (C₂H₆), calculate the following:

• Number of moles of carbon atoms.
• Number of moles of hydrogen atoms.
• Number of molecules of ethane.

Answer:

• 1 mole of C2H6 contains 2 moles of carbon atoms

: Number of moles of carbon atoms in 3 moles of C2H6

= 3 x 6 = 18

• 1 mole of C2H6 contains 6.023 x 10²³ molecules of ethane

:Number of molecules in 3 moles of C2H6

= 3 x 6.022 x 10²³ = 18.069 x 10²³

 

Question: 11 What is the concentration of sugar in molL-1. If its 20 g are dissolved in enough water to make a final volume up to 2L?

Answer:
Molarity of a solution is given by:
= Number of moles of solute / Volume of solution in Litres
= Mass of sugar / molar mass of sugar
2 L
= 20 g / [(12 x 12) + (1 x 22) + (11 x 16)]g
2 L
= 20g / 342 g
2L
= 0.0585 mol / 2L
= : Molar concentration of sugar = 0.02925 mol /L

 

Question:12 If the density of methanol is 0.793 kg L-1, what is its volume needed for making 2.5 L of its 0.25M solution?

Answer:
Molar mass of methanol(CH2OH) = (1 x 12) + (4 x 1) + (1 x 16)
= 32 g mol-1
= 0.032 kg mol-1
Molarity of the methanol solution = 0.793kg L-1 / 0.032 kg mol-1
= 24.78 mol L-1
(Since density is mass per unit volume)
Applying, M1V1 = M2V2
(Given solution)(Solution to be prepared)
V1 = 0.0252 L
V1 = 25.22Ml

 

Question:13 Pressure is determined as force per unit area of the surface. The SI unit of pressure, pascal is as shown below:
1 Pa = 1 N m-2
If mass of air at sea level is 1034 g cm-2, calculate the pressure in pascal.

Answer:
Pressure is defined as force acting per unit area of the surface.
P = F / A
= 1034g x 9.8ms-1 x 1kg x (100)2cm2
Cm2 1000g 1 m2
= 1.01332 x 106kg m-1s-2
We know,
1N = 1kg ms-2
Then,
1 Pa = 1Nm-2 1Kg m-1s-2
: Pressure = 1.01332 x 106 Pa

 

Question:14 What is the SI unit of mass? How is it defined?

Answer:
The SI unit of mass is kilogram (kg). 1 kilogram is defined as the mass equal to the mass of international prototype of kilogram.

 

Question:15 Match the following prefixes with their multiples:
Prefixes Multiples
i.) Micro 106
ii.) Deca 109
iii.) Mega 10-6
iv.) Giga 10-15
v.) femto 10

Answer:
Prefixes
Multiples
micro
10-6
Deca
10
Mega
106
Giga
109
Femto
10-15

Question:16 What do you mean by significant figures?

Answer:
Significant figures are those meaningful digits that are known with certainty. They indicate uncertainty in an experiment or calculated value. For example, if 15.6 mL is the result of an experiment, tyhen 15 is certain while 6 is uncertain and the total number of significant figures are 3.
Hence, significant figures are defined as the total number of digits in a number including the last digit that represents the uncertainity of the result.

 

Question:17 A sample of drinking water was found to be severely contaminated with chloroform. CHCl3, supposed to be carcinogenic in nature. The level of contamination was 15 ppm (by mass).
i.) Express this in percent by mass.
ii.) Determine the molality of chloroform in the water sample.

Answer:
i.) 1 ppm is equivalent ti 1 part out of 1 million (1060 parts.
: Mass percent of 15 ppm chloroform in water
= 15 x 100 / 106
= 15 x 10-3%
ii.) 100 g of the sample contains 1.5 x 10-3g of CHCl3
= 1000 g of the sample contains 1.5 x 10-2 g of CHCl3
Molality of chloroform in water
= 1.5 x 10-2 g / Molar mass of CHCl3
Molar mass of CHCl3 = 12.00 + 1.00 + 3(35.5)
= 119.5 g / mol
Molality of chjloroform in water = 0.0125 x 10-2m
= 1.25 x 10-4m

 

Question:18 Express the following in scientific notation:
i.) 0.0048
ii.) 234,000
iii.) 8008
iv.) 500.0
v.) 6.0012

Answer:
i.) 0.0048 = 4.8 x 10-3
ii.) 234,000 = 2.34 x 105
iii.) 8008 = 8.008 x 103
iv.) 500.0 = 5.000 x 102
v.) 6.0012 = 6.0012 x 100

 

Question:19 How many significant figures are present in the following:
i.) 0.0025
ii.) 208
iii.) 5005
iv.) 126,000
v.) 500.0
vi.) 2.0034

Answer:
i.) 0.0025
There are two significant figures.
ii.) 208
There are 3 significant figures
iii.) 5005
There are 4 significant figures
iv.) 126.000
There are 3 significant figures
v.) 500.0
There are 4 significant figures
vi.) 2.0034
There are 5 significant figures.

 

Question:20 Round up the following upto three significant figures:
i.) 34.216
ii.) 10.4107
iii.) 0.04597
iv.) 2808

Answer:
i.) 34.216
ii.) 10.4107
iii.) 0.04597
iv.) 2808

Question:21 The following data obtained when dinitrogen and dioxygen react together to form different compound:
Mass of dinitrogen
Mass of dioxygen
14 g
16 g
14 g
32 g
28 g
32 g
28 g
80 g
a.) Which law of chemical combination is obeyed by the above experimental data? Give statement.
b.) Fill in the blanks in the following conversions:
i.) 1 km = ———mm = ………….. pm
ii.) 1 mg = ………..kg = ……………ng
iii.) 1 ml = …………L = ……………..dm3

Answer:
Let us fix 14 parts by weight of nitrogen as fixed weight.
Now let us calculate the weights of oxygen which combine with 14 parts by weight of nitrogen
S No
No. of parts by weight of nitrogen
No. of parts by weight of oxygen
14 parts of nitrogen as fixed weight
No. of parts by weight of oxygen which combine with 14 parts by weight of nitrogen
1
14 g
16 g
14 g
16
2
14 g
32 g
14 g
32
3
28 g
32 g
14 g
32
4
28 g
80 g
14 g
80
(a) If we fix the mass of dinitrogen at 14 g, then the masses of dioxygen that will combine with the fixed mass of dinitrogen are 16 g, 32 g, 32 g, and 80 g.
The masses of dioxygen bear a whole number ratio of 1:2:2:5. Hence, the given experimental data obeys the law of multiple proportions.
This law was given by Dalton in 1804. The law states that if two elements combine to form 2 or more compound, then the weight of one element which combines a fixed weight of other element in these compounds, bears a simple whole number ratio by weight.
(b) (i) We know 1km=1000m
Or 1m = 1000 mm
Therefore 1km = 1000x 1000mm= 106 mm
1 km = 1 km × 1000 m / 1 km x 1 pm / 10-12 m
1 km = 1015 pm
Hence, 1 km = 106 mm = 1015 pm
(ii) We know 1kg = 1000mg
Or 1000mg= 1kg
Or 1mg= 1/1000* 1= 0.01 kg
1 mg = 1 mg × 1g / 1000mg x 1 ng / 10-9g
⇒ 1 mg = 106 ng
1 mg = 10-6 kg = 106 ng
(iii) We know 1000 ml=l L
Or 1ml=1/1000*1= 0.01L
1 mL = 1 cm3 = 1 cm3
⇒ 1 mL = 10-3 dm3
1 mL = 10-3 L = 10-3 dm3

 

Question:22 If the speed of light is 3.0 x 108m s-1. Calculate the distance covered by light in 2.00ns.

Answer:
According to the equation:
Time taken to cover the distance = 2.00 ns
= 2.00 x 10-9s
Speed of light = 3 x 108ms-1
Distance travelled by light in 2.00 ns
= Speed of light x time taken
= (3.0 x 108 ms-1) (2.00 x 10-9)
= 6.00 x 10-1 m
0.600 m

 

Question:23 In a reaction
A + B2 -AB2
Identify the limiting reagent, if any, in the following reaction mixtures.
i.) 300 atoms of A + 200 molecules of B
ii.) 2 mol A + 3 mol B
iii.) 100 atom of A + 100 molecules of B
iv.) 5 mol A + 2.5 mol B
v.) 2.5 mol A + 5 mol B

Answer:
A limiting reagent determines the extentof a reaction. It is the reactant which is the first to get consumed during a reaction, thereby causing the reaction to stop and limiting tha amount of product formed.
(i) According to the given reaction, 1 atom of A reacts with 1 molecule of B. Thus, 200 molecules of B will react with 200 atoms of A, thereby leaving 100 atoms of A unused. Hence, B is the limiting reagent. Here atom B is in lesser amount(200).
(ii) According to the reaction, 1 mol of A reacts with 1 mol of B. Thus, 2 mol of A will react with only 2 mol of B. As a result, 1 mol of A will not be consumed. Hence, A is the limiting reagent.
(iii) According to the given reaction, 1 atom of A combines with 1 molecule of B. Thus, all 100 atoms of A will combine with all 100 molecules of B. Hence, the mixture is stoichiometric where no limiting reagent is present.
(iv) 1 mol of atom A combines with 1 mol of molecule B. Thus, 2.5 mol of B will combine with only 2.5 mol of A. As a result, 2.5 mol of A will be left as such. Hence, B is the limiting reagent because B is less as compared to A
(v) According to the reaction, 1 mol of atom A combines with 1 mol of molecule B. Thus, 2.5 mol of A will combine with only 2.5 mol of B and the remaining 2.5 mol of B will be left as such. Hence, A is the limiting reagent

 

Question:24 Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation:
N2(g) + H2(g)  2NH3 (g)
i.) Calculate the mass of ammonia produced if 2.00 x 103g dinitrogen reacts with 1.00 x 103 g of hydrogen.
ii.) Will any of the reactants remain unreacted?
iii.) If yes, which one and what would be its mass?

Answere:
(i) Balancing the given chemical equation,
N2(g) + H2(g)  2NH3 (g)
Total mass of Ammonia = 2((14) +3(1)) = 34 g
From the chemical equation, we can write
28gm of N2 reacts with 6gm of H2 to produce ammonia= 34g
Or 1 gm of N2 reacts with 1gm of H2 to produce ammonia= 34/28*1
Or when 2.00 x 103 g of N2 reacts with 1.00 x 103 gm of H2 to produce ammonia
=34/28 *2.00 x 103 = 2428.57g
Hence 2.00 × 103 g of dinitrogen will react with 1.00 x 103 g of dihydrogen to give 2428.57 g of ammonia
Given, Amount of dihydrogen = 1.00 × 103 g
Hence, N2 is the limiting reagent.
(ii) N2 is the limiting reagent and H2 is the excess reagent. Hence, H2 will remain unreacted.
(iii) Mass of dihydrogen left unreacted = 1.00 × 103 g – 428.6 g
= 571.4 g

 

Question:25 How are 0.50 mol Na2CO3 and 0.50 M Na2CO3 different?

Answer:
Molar mass of Na2CO3 = (2 x 23) + 12.00 + (3 x 6)
= 106 g mol-1
Now, 1 mole of Na2CO3 means 106 g of Na2CO3
: 0.5 mol of Na2CO3 = 106 g x 0.5 mol / 1 mole
= 53 g Na2CO3
= 0.50 M of Na2CO3 = 0.50 mol / L Na2CO3
Hence, 0.50 mol of Na2CO3 is present in 1 L of water or 53 g Na2CO3 is present in 1 L of water.

 

Question: 26 If ten volumes of dihydrogen gas reacts with five volume of dioxygen gas, how many volumes of water vapour would be produced?

Answer:
Reaction of dihydrogen with dioxygen can be written as:
2H2(g) + O29g)  2H2O(g)
Now, two volumes of dihydrogen react with one volume of dihydrogen to produce two volumes of water vapour
Hence, ten volumes of dihydrogen will react with five volumes of dioxygen to produce ten volumes of water vapour.

 

Question:27 Convert the following in basic units:
i.) 28.7 pm
ii.) 15.15 pm
iii.) 25365 mg

Answer:
(i) 28.7 pm:
1 pm = 10-12 m
28.7 pm = 28.7 × 10-12 m
= 2.87 × 10-11 m
(ii) 15.15 pm:
1 pm = 10-12 m
15.15 pm = 15.15 × 10-12 m
= 1.515 × 10-12 m
(iii) 25365 mg:
1 mg = 0.01 kg
Therefore 25365 mg = 0.01/1 x 25365= 253.65 kg

 

Question:28 Which one of the following will have largest no. of atoms:
i.) 1 g Au (s)
ii.) 1 g Na (s)
iii.) 1 g Li (s)
iv.) 1 g Cl2 (g)

Answer:
(i) Gram atomic mass of Au= 197 g
Or
197g of Au contains = 6.022 x 1023
Therefore 1gm of Au contains = 6.022 x 1023/197*1 = 3.06 x 1021 atoms
(ii) Gram atomic mass of Na = 23 g
Or
23 g of Na contains atoms = 6.022x 1023
Or
1gm of Na contains atoms = 6.022×1023 /23 *1 = 26.2 x1021 atoms
(iii) Gram atomic mass of Li = 7
Or
7g of Li contains atoms = 6.022 x 1023
Or
1g of Li contains atoms = 6.022 x 1023/7 *1= 86.0 x 1021 atoms
(iv) Gram atomic mass of Cl = 71 Or 71g of Cl contains atoms = 6.022×1023
Or
1 g of Cl contains atoms = 6.022×1023 /71 * 1= 8.48 x 1021 atoms
Hence, 1 g of Li (s) will have the largest number of atoms

 

Question:29 Calculate the molarity of a solution of ethanol in water in which the mole fraction of ethanol is 0.040 (assume the density of water to be one).

Answer:
Mole fraction of C2H5OH= Number of moles of C2H5OH / Number of moles of solution
Let the moles of C2H5OH= X
Now density of water = 1 (given)
And the weight of 1000ml of water = volume * density (from density = mass/volume)
= 1000 x 1=1000g
Therefore moles of water = 1000/18 = 55.55 mol (18g is molecular mass of water)
Also mole fraction of C2H5OH= 0.040 (given)
Putting the values in equation 1,we get
= 0.040 = X/X + 55.55
=0.040X + 2.222 = X
OR
X= 2.3145 mol
Molarity of solution = 2.314 M

 

Question:30 What will be the mass of one 12C atom in g?

Answer:
1 mole of carbon atoms = 6.022 x 1023 atoms of carbon
= 12 g of carbon
: Mass of one 12C atom = 12g/ 6.022 x 1023
= 1.993 x 10-23g

Question:31 How many significant figures should be present in the answer of the following calculations?
i.) 0.02856 x 298.15 x 0.112
0.5785
ii.) 5 x 5.364
iii.) 0.0125 + 0.7864 + 0.0215

Answer:
(i) Least precise term i.e. 0.112 is having 3 significant digits.
∴ There will be 3 significant figures in the calculation.
(ii) 5.364 is having 4 significant figures.
∴ There will be 4 significant figures in the calculation.
(iii) Least number of decimal places in each term is 4.
∴ There will be 4 significant figures

 

Question:32 Use the data given in the following table to calculate the molar mass of naturally occurring argon isotopes:
Isotope
Isotopic molar mass
Abundance
36Ar
35.96755 g mol-1
0.337%
38Ar
37.96272 g mol-1
0.063%
40Ar
39.9624 g mol-1
99.600%

Answer:
Molar mass of argon
= [ (35.96755 x 0.337/100) + (37.96272 x 0.063/100) + (39.9624 x 90.60/100) ] g mol-1
= [ 0.121 + 0.0024 + 39.802 ] gmol-1
= 39.947 gmol-1

 

Question:33 Calculate the no. of atoms in each of the following :
i.) 52 moles of Ar
ii.) 52 u of He
iii.) 52 g of He

Answer:
(i) 1 mole of Ar = 6.022 × 1023 atoms of Ar
52 mol of Ar = 52 × 6.022 × 1023 atoms of Ar
= 3.131 × 1025 atoms of Ar
(ii) Atomic mass of He = 4amu
Or
4amu is the mass of He atoms = 1
Therefore 52 amu is the mass of He atoms= ¼*52 = 13 atoms of He
(iii) Gram atomic mass of He = 4g
Or
4g of He contains = 6.022x 1023 atoms
Therefore 52 g of He contains = 6.022x 1023 /4 * 52 = 7.83 x 1024 atoms

 

Question:34 A welding fuel gas contains carbon and hydrogen only. Burning a small sample of it in oxygen gives 3.38 g carbon dioxide, 0.690 g of water and no other products. A volume of 10.0 L (measured at STP) of this welding gas is found to weigh 11.6 g. Calculate:
i.) Empirical formula
ii.) Molar mass of the gas
iii.) Molecular formula

Answer:
(i) Mass of carbon in 3.38 g of CO2 = 3.38 g/44 x 12 = 0.922 g
Mass of hydrogen in 0.690 g of H2O = 0.690 g/18 x 2 = 0.077 g
Total mass of the sample burnt = 0.922 g + 0.077 g = 0.999 g
Percentage of carbon in the fuel = {0.922}/{0.999 g} x 100 = 92.29%
Percentage of hydrogen in the fuel = {0.077 g}/{0.999 g} x 100 = 7.71%
Element
Mass percent
Atomic mass
Relative no. of atoms
Simple atomic ratio
Carbon (C)
92.29
12.0
92.29 / 12.0 = 7.69
7.69 / 7.69 = 1
Hydrogen
7.71
1.0
7.71 / 1.0 = 7.71
7.71 / 7.69 = 1
Therefore, empirical formula of the compound = CH
(ii) Volume of the gaseous fuel = 11.6 g
Molar mass of the fuel = {11.6 g}/{10.0 L} x 22.4 L/ml = 26.0 g mol-1
(iii) Empirical formula mass of the fuel = (12 + 1) g mol-1 = 13 g mol-1
Molar mass of the fuel = 26.0 g mol-1 n = {26.0 g mol-1}/{13 g mol-1} = 2
Molecular formula of the fuel = 2 x Empirical formula = 2 x CH = C2H2

 

Question:35 Calcium carbonate reacts with aqueous HCl to give CaCl2 and CO2 according to the reaction, CaCO3 (s) + 2 HCl (aq)  CaCl2(aq) + CO2(g) + H2O(l)
What mass of CaCO3 is required to react completely with 25 ml of 0.75 M HCl?
Answer:
0.75 M of HCl = 0.75 mol of HCl are present in 1 L of water
= [(0.75 mol ) x (36.5 g mol-1)] HCl is present in 1 L of water
= 27.375 g of HCl is present in 1 L of water
Thus, 1000 mL of solution
= 27.375g x 25mL / 1000 Ml
= 0.6844 g
From the given chemical equation
CaCO2(s) + 2HCl(aq)  CaCl2(aq) + CO2(g) + H2O(l)
2 mol of HCl (2 x 36.5 = 71 g) react wuth 1 mol of CaCO3 (100g).
: Amount of CaCO3 that will react with 0.6844 g = 100 x 0.6844 g / 71
= 0.9639 g

 

Question:36 Chlorine is prepared in the laboratory by treating manganese dioxide (MnO2) with aqueous hydrochloric acid according to the reaction
4HCl(aq) + MnO2(s)  2H2O(l) + MnCl2(aq) + Cl2(g)
How many grams of HCl react with 5.0 g of manganese dioxide?

Answer:
1 mol [55 + 2 x 16 = 87 g] MnO2 reacts completely with 4 mol[4 x 36.5 = 146 g] of HCl
: 50 g of MnO2 will react with
= 146g x 5.0 g / 87 g
= 8.4 g of HCl
Hence, 8.4 g of HCl will react with 5.0 g of manganese dioxide.

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