Class 10th Science Tamilnadu Board Solution
Part-a- From the given examples, form the pair of isotopes and the pair of isobars: 18Ar^40 ,…
- Molecular mass of Nitrogen is 28. Its atomic mass is 14. Find the atomicity of Nitrogen.…
- Gram molecular mass of Oxygen is 32 g. Density of Oxygen is 1.429 g/litre. Find the gram…
- ‘Cl’ represents Chlorine atom, ‘Cl2’ represents Chlorine molecule. List out any two…
- Calculate the gram molecular mass of water from the values of gram atomic mass of Hydrogen…
- One mole of any substance contains 6.023 x 10^23 particles. If 3.0115 x 10^23 particles…
- _________ have equal number of neutrons. i) Isobars ii) Isotones iii) Isotopes iv) Mass…
- Classify the following based on atomicity: i) Chlorine ii) Neon iii) Phosphorous iv) Ozone…
- Identify and correct the mistake in each of the following: i) The molar volume of gas at…
- Give a single term substitute for each of the following: i) 6.023 x 10^23 molecules ii)…
Part-b- Modern atomic theory takes up the wave concept, principle of uncertainty and other latest…
- How will you establish the relation between vapour density and molecular mass of a gas by…
- Calculate the number of moles in: i) 12.046 x 10^23 atoms of Copper ii) 27.95g of Iron…
- Find the gram molecular mass of the following from the data given: i) H2O ii) CO2 iii)…
- Complete the table given below:
- Calculate the number of water molecules present in one drop of water which weighs 0.18 g.…
- Fill in the blanks using the given data: The formula of Calcium oxide is CaO. The atomic…
- How many grams are there in: i) 5 moles of water ii) 2 moles of Ammonia iii) 2 moles of…
Part-c- When ammonia reacts with hydrogen chloride gas, it produces white fumes of ammonium…
- Nitro glycerine is used as an explosive. The equation for the explosive reaction is…
- Sodium bi carbonate breaks down on heating: 2NaHCO3 Na2CO3 + H2O + CO2 (Atomic mass of Na…
- 40 g of calcium was extracted from 56 g of calcium oxide (Atomic mass of Ca= 40, O=16) i)…
- How many grams are there in the following? i) 1 mole of chlorine molecule, Cl2 ii) 2 moles…
- Find how many moles of atoms are there in: i) 2 g of nitrogen. ii) 23 g of sodium iii) 40…
- From the given examples, form the pair of isotopes and the pair of isobars: 18Ar^40 ,…
- Molecular mass of Nitrogen is 28. Its atomic mass is 14. Find the atomicity of Nitrogen.…
- Gram molecular mass of Oxygen is 32 g. Density of Oxygen is 1.429 g/litre. Find the gram…
- ‘Cl’ represents Chlorine atom, ‘Cl2’ represents Chlorine molecule. List out any two…
- Calculate the gram molecular mass of water from the values of gram atomic mass of Hydrogen…
- One mole of any substance contains 6.023 x 10^23 particles. If 3.0115 x 10^23 particles…
- _________ have equal number of neutrons. i) Isobars ii) Isotones iii) Isotopes iv) Mass…
- Classify the following based on atomicity: i) Chlorine ii) Neon iii) Phosphorous iv) Ozone…
- Identify and correct the mistake in each of the following: i) The molar volume of gas at…
- Give a single term substitute for each of the following: i) 6.023 x 10^23 molecules ii)…
- Modern atomic theory takes up the wave concept, principle of uncertainty and other latest…
- How will you establish the relation between vapour density and molecular mass of a gas by…
- Calculate the number of moles in: i) 12.046 x 10^23 atoms of Copper ii) 27.95g of Iron…
- Find the gram molecular mass of the following from the data given: i) H2O ii) CO2 iii)…
- Complete the table given below:
- Calculate the number of water molecules present in one drop of water which weighs 0.18 g.…
- Fill in the blanks using the given data: The formula of Calcium oxide is CaO. The atomic…
- How many grams are there in: i) 5 moles of water ii) 2 moles of Ammonia iii) 2 moles of…
- When ammonia reacts with hydrogen chloride gas, it produces white fumes of ammonium…
- Nitro glycerine is used as an explosive. The equation for the explosive reaction is…
- Sodium bi carbonate breaks down on heating: 2NaHCO3 Na2CO3 + H2O + CO2 (Atomic mass of Na…
- 40 g of calcium was extracted from 56 g of calcium oxide (Atomic mass of Ca= 40, O=16) i)…
- How many grams are there in the following? i) 1 mole of chlorine molecule, Cl2 ii) 2 moles…
- Find how many moles of atoms are there in: i) 2 g of nitrogen. ii) 23 g of sodium iii) 40…
Part-a
Question 1.From the given examples, form the pair of isotopes and the pair of isobars:
18Ar40, 17Cl35, 20Ca40, 17Cl37
Answer:● Isotopes are the atoms of same chemical element having different
atomic mass. This means they differ in neutron number. For ex- 17Cl35 and 17Cl37. Here both atoms are chlorine atoms and have atomic number 17. So, each atom has 17 electrons and 17 protons. But the former one has atomic mass 35 and the latter one has atomic mass 37. This implies that former one has 18 neutrons (35-17) and latter one has 20 neutrons (37-17). Hence, they are isotopes.
● Isobars are the atoms of different elements having same atomic mass.
This implies that the sum of protons and neutrons in each atom is same. For ex- 18Ar40 and 20Ca40. Here, the former one is argon atom and latter one is calcium. Their atomic numbers are different. But their atomic mass is same i.e. 40. This implies that the number of nucleons in both atoms is same, even though the proton, electron and neutron numbers are different.
Question 2.Molecular mass of Nitrogen is 28. Its atomic mass is 14. Find the atomicity of Nitrogen.
Answer:Atomicity is the number of atoms in the molecule of an element. Molecular mass is calculated by adding up the masses of respective atoms present in the molecule. Nitrogen molecule contains only nitrogen atoms. Given -
Mass of molecule of nitrogen = 28
Mass of atom of nitrogen = 14
Let number of atoms in the molecule = x
So,
Hence, the atomicity of nitrogen is 2. 2 atoms of nitrogen make one
molecule of nitrogen.
Question 3.Gram molecular mass of Oxygen is 32 g. Density of Oxygen is 1.429 g/litre. Find the gram molar volume of Oxygen.
Answer:Given - Gram molecular mass of Oxygen = 32 g
Density of Oxygen = 1.429 g/litre
Gram molar volume of Oxygen = ?
Formula used is -
Question 4.‘Cl’ represents Chlorine atom, ‘Cl2’ represents Chlorine molecule.
List out any two differences between atoms and molecules.
Answer:
Note –
Atoms combine to form molecules.
Question 5.Calculate the gram molecular mass of water from the values of gram atomic mass of Hydrogen and of Oxygen.
Gram atomic mass of Hydrogen = 1 g
Gram atomic mass of Oxygen = 16 g
Answer:If the molecular mass of a given substance is expressed in grams, it is known as gram molecular mass of that substance. Molecular mass is the sum of the atomic masses of all the atoms present in one molecule of the substance.
One molecule of water is H2O, which contains 2 hydrogen and one oxygen atoms. So, molecular mass is sum of atomic masses of hydrogen and oxygen atoms.
Gram molecular mass of water is 18g.
Question 6.One mole of any substance contains 6.023 x 1023particles.
If 3.0115 x 1023 particles are present in CO2, find the number of moles.
Answer:Number of particles in one mole of any substance is 6.023 x 1023
Note:
1. If a compound or molecular substance is taken, like CO2, N2 etc, then 1
mole of the substance contains Avogadro number of molecules. 1 mole contains the mass equal to molecular weight of substance.
2. If a element is taken like C, S, Fe, then 1 mole contains Avogadro
number of atoms. 1 mole contains the mass equal to atomic weight of substance.
Question 7._________ have equal number of neutrons.
i) Isobars ii) Isotones
iii) Isotopes iv) Mass Numbers
Answer:isotones
These are the atoms of different elements with same number of neutrons. Example : 6C13 and 7N14
Number of neutrons is obtained by subtracting atomic number from atomic mass number.
Number of neutrons in 6C13 is (13-6) 7.
Number of neutrons in 7N14 is (14-7) 7.
● Isobars are the atoms of different elements having same mass number but different atomic numbers.
● Isotopes are the atoms of same element with same atomic number but
different mass number.
● Mass numbers is the sum of protons and neutrons.
Question 8.Classify the following based on atomicity:
i) Chlorine ii) Neon
iii) Phosphorous iv) Ozone
Answer:● chlorine is diatomic because its molecule contains 2 atoms of chlorine. Cl2
● neon is monoatomic because its molecule contains 1 atom of neon. Ne
● Phosphorous is polyatomic because its molecule contains 4 atoms of
phosphorous. If a molecule contains more than 3 atoms in its molecule its polyatomic. P4
● ozone is triatomic because its molecule contains 3 atoms of oxygen. O3
Question 9.Identify and correct the mistake in each of the following:
i) The molar volume of gas at STP is 22.4 cm3.
ii) 2 x R.M.M. = V.D.
iii) An atom cannot exist independently.
iv) The ratio of atoms in a molecule may be integral or simple or may not be fixed.
v) H2O is a homo atomic molecule.
Answer:(i) The molar volume of gas at STP is 22.4 litres (not cm3.)
(ii) 2 x V.D = R.M.M
(iii) An atom may or may not exist independently. Atoms like Fe, Na
can exist independently.
(iv) The ratio of atoms in a molecule may be fixed and integral but
may not be simple.
(v) H2O is a hetero atomic molecule. It contains more than one type
of atoms i.e hydrogen and oxygen. So, it’s a hetero atomic molecule , not homo atomic molecule.
Question 10.Give a single term substitute for each of the following:
i) 6.023 x 1023 molecules ii) 22.4 litres of gas at STP
iii) 1/12th part of the mass of one atom of carbon
iv) The half of relative molecular mass
v) Molecular mass / atomic mass
Answer:(i) 1 mole of a compound or molecular substance / Avogadro number of molecules.
(ii) Molar volume
(iii) One atomic mass unit
(iv) Vapour density
(v) atomicity
From the given examples, form the pair of isotopes and the pair of isobars:
18Ar40, 17Cl35, 20Ca40, 17Cl37
Answer:
● Isotopes are the atoms of same chemical element having different
atomic mass. This means they differ in neutron number. For ex- 17Cl35 and 17Cl37. Here both atoms are chlorine atoms and have atomic number 17. So, each atom has 17 electrons and 17 protons. But the former one has atomic mass 35 and the latter one has atomic mass 37. This implies that former one has 18 neutrons (35-17) and latter one has 20 neutrons (37-17). Hence, they are isotopes.
● Isobars are the atoms of different elements having same atomic mass.
This implies that the sum of protons and neutrons in each atom is same. For ex- 18Ar40 and 20Ca40. Here, the former one is argon atom and latter one is calcium. Their atomic numbers are different. But their atomic mass is same i.e. 40. This implies that the number of nucleons in both atoms is same, even though the proton, electron and neutron numbers are different.
Question 2.
Molecular mass of Nitrogen is 28. Its atomic mass is 14. Find the atomicity of Nitrogen.
Answer:
Atomicity is the number of atoms in the molecule of an element. Molecular mass is calculated by adding up the masses of respective atoms present in the molecule. Nitrogen molecule contains only nitrogen atoms. Given -
Mass of molecule of nitrogen = 28
Mass of atom of nitrogen = 14
Let number of atoms in the molecule = x
So,
Hence, the atomicity of nitrogen is 2. 2 atoms of nitrogen make one
molecule of nitrogen.
Question 3.
Gram molecular mass of Oxygen is 32 g. Density of Oxygen is 1.429 g/litre. Find the gram molar volume of Oxygen.
Answer:
Given - Gram molecular mass of Oxygen = 32 g
Density of Oxygen = 1.429 g/litre
Gram molar volume of Oxygen = ?
Formula used is -
Question 4.
‘Cl’ represents Chlorine atom, ‘Cl2’ represents Chlorine molecule.
List out any two differences between atoms and molecules.
Answer:
Note –
Atoms combine to form molecules.
Question 5.
Calculate the gram molecular mass of water from the values of gram atomic mass of Hydrogen and of Oxygen.
Gram atomic mass of Hydrogen = 1 g
Gram atomic mass of Oxygen = 16 g
Answer:
If the molecular mass of a given substance is expressed in grams, it is known as gram molecular mass of that substance. Molecular mass is the sum of the atomic masses of all the atoms present in one molecule of the substance.
One molecule of water is H2O, which contains 2 hydrogen and one oxygen atoms. So, molecular mass is sum of atomic masses of hydrogen and oxygen atoms.
Gram molecular mass of water is 18g.
Question 6.
One mole of any substance contains 6.023 x 1023particles.
If 3.0115 x 1023 particles are present in CO2, find the number of moles.
Answer:
Number of particles in one mole of any substance is 6.023 x 1023
Note:
1. If a compound or molecular substance is taken, like CO2, N2 etc, then 1
mole of the substance contains Avogadro number of molecules. 1 mole contains the mass equal to molecular weight of substance.
2. If a element is taken like C, S, Fe, then 1 mole contains Avogadro
number of atoms. 1 mole contains the mass equal to atomic weight of substance.
Question 7.
_________ have equal number of neutrons.
i) Isobars ii) Isotones
iii) Isotopes iv) Mass Numbers
Answer:
isotones
These are the atoms of different elements with same number of neutrons. Example : 6C13 and 7N14
Number of neutrons is obtained by subtracting atomic number from atomic mass number.
Number of neutrons in 6C13 is (13-6) 7.
Number of neutrons in 7N14 is (14-7) 7.
● Isobars are the atoms of different elements having same mass number but different atomic numbers.
● Isotopes are the atoms of same element with same atomic number but
different mass number.
● Mass numbers is the sum of protons and neutrons.
Question 8.
Classify the following based on atomicity:
i) Chlorine ii) Neon
iii) Phosphorous iv) Ozone
Answer:
● chlorine is diatomic because its molecule contains 2 atoms of chlorine. Cl2
● neon is monoatomic because its molecule contains 1 atom of neon. Ne
● Phosphorous is polyatomic because its molecule contains 4 atoms of
phosphorous. If a molecule contains more than 3 atoms in its molecule its polyatomic. P4
● ozone is triatomic because its molecule contains 3 atoms of oxygen. O3
Question 9.
Identify and correct the mistake in each of the following:
i) The molar volume of gas at STP is 22.4 cm3.
ii) 2 x R.M.M. = V.D.
iii) An atom cannot exist independently.
iv) The ratio of atoms in a molecule may be integral or simple or may not be fixed.
v) H2O is a homo atomic molecule.
Answer:
(i) The molar volume of gas at STP is 22.4 litres (not cm3.)
(ii) 2 x V.D = R.M.M
(iii) An atom may or may not exist independently. Atoms like Fe, Na
can exist independently.
(iv) The ratio of atoms in a molecule may be fixed and integral but
may not be simple.
(v) H2O is a hetero atomic molecule. It contains more than one type
of atoms i.e hydrogen and oxygen. So, it’s a hetero atomic molecule , not homo atomic molecule.
Question 10.
Give a single term substitute for each of the following:
i) 6.023 x 1023 molecules ii) 22.4 litres of gas at STP
iii) 1/12th part of the mass of one atom of carbon
iv) The half of relative molecular mass
v) Molecular mass / atomic mass
Answer:
(i) 1 mole of a compound or molecular substance / Avogadro number of molecules.
(ii) Molar volume
(iii) One atomic mass unit
(iv) Vapour density
(v) atomicity
Part-b
Question 1.Modern atomic theory takes up the wave concept, principle of uncertainty and other latest discoveries to give a clear-cut picture about an atom. State the findings of modern atomic theory.
Answer:● An atom is the smallest particle which takes part in chemical reaction.
● An atom is considered to be a divisible particle.
● The atoms of the same element may not be similar in all respects.
ex: Isotopes (17Cl35, 17Cl37 )
● The atoms of different elements may be similar in some respects.
ex. Isobars ( 18Ar40 , 20Ca40 )
● The ratio of atoms in a molecule may be fixed and integral but may not be simple. Ex.C12H22O11 is not a simple ratio. (Sucrose)
● The atoms of one element can be changed into the atoms of another element by transmutation.
● The mass of an atom can be converted into energy. This is in accordance with Einstein’s equation E = mc2 where E = energy, m = mass and c = velocity of light
Question 2.How will you establish the relation between vapour density and molecular mass of a gas by applying Avogadro’s law?
Answer:Relative Molecular Mass: It is defined as the ratio of the mass of 1 molecule of the gas or vapour to the mass of 1 atom of hydrogen.
Vapour Density (V.D): It is defined as the ratio of the mass of a certain volume of the gas or vapour to the mass of the same volume of hydrogen at the same temperature and pressure.
Applying Avogadro’s Law,
Since hydrogen is diatomic,
2 x V.D = relative molecular mass of a gas or vapour
2 x Vapour density = Relative molecular mass
Question 3.Calculate the number of moles in:
i) 12.046 x 1023 atoms of Copper
ii) 27.95g of Iron
iii) 1.51 x 1023molecules of CO2
Answer:we know that to find the number of moles, the following formulae are used:
(i) Using formula 3,
So, 2 moles of copper contain 12.046 x 1023 atoms of copper.
(ii) Using formula 1,
So, 0.5 moles consist of 27.95 grams of iron.
(iii) Using formula 4,
So, 0.25 moles of CO2 consists of 1.51 x 1023 molecules.
Note:
1. If a compound or molecular substance is taken, like CO2, N2 etc, then 1
a mole of the substance contains Avogadro number of molecules. 1 mole contains the mass equal to the molecular weight of the substance.
2. If an element is taken like C, S, Fe, then 1 mole contains Avogadro
number of atoms. 1 mole contains the mass equal to the atomic weight of the substance.
Question 4.Find the gram molecular mass of the following from the data given:
i) H2O ii) CO2 iii) NaOH iv) NO2 v) H2SO4
Answer:Molecular mass is the sum of the atomic masses of all the atoms present in one molecule of the substance.
1. H2O = (1gX2) + 16g = 18g
2. CO2 = 12g + (2 x16g) = 12 + 32 = 44g
3. NaOH = 23g + 16g + 1g = 40g
4. NO2 = 14 + (2 x 16) = 46g
5. H2SO4 = (1gx2) + 32g + (4x16g) = 98g
Question 5.Complete the table given below:
Answer:Formula used is
So, the complete table is
Question 6.Calculate the number of water molecules present in one drop of water which weighs 0.18 g.
Answer:According to mole concept we know that gram molecular weight of any compound consists of Avogadro number of molecules.
This implies that 18 grams of water consists 6.023 x 1023 molecules of water.
18 grams 
6.023 x 1023 molecules
0.18 grams ?
Question 7.Fill in the blanks using the given data:
The formula of Calcium oxide is CaO. The atomic mass of Ca is 40, Oxygen is 16 and Carbon is 12.
i) 1 mole of Ca ( ____g) and 1 mole of Oxygen atom ( ___g) combine to form _____mole of CaO ( ____g).
ii) 1 mole of Ca ( ___g) and 1 mole of C ( ___g) and 3 moles of Oxygen atom ( ___g) combine to form 1 mole of CaCO3 ( ___g)
Answer:i) 1 mole of Ca ( 40 g) and 1 mole of an Oxygen atom ( 16 g) combine to form 1 mole of CaO ( 56 g).
ii) 1 mole of Ca ( 40 g) and 1 mole of C ( 12 g) and 3 moles of an Oxygen atom ( 3x16 = 48 g) combine to form 1 mole of CaCO3 ( 100 g)
Note:
1. If a compound or molecular substance is taken, like CO2, N2 etc, then 1
a mole of the substance contains Avogadro number of molecules. 1 mole contains the mass equal to the molecular weight of the substance.
2. If an element is taken like C, S, Fe, then 1 mole contains Avogadro
number of atoms. 1 mole contains the mass equal to the atomic weight of the substance.
So, 1 mole of Ca is 40 grams, 1 mole of O atom is 16 grams and 1 mole of C is 12 grams of C. 1 mole of CaO is 56 grams (40+16) of CaO and 1 mole of CaCO3 is 100 grams ( 40+12+48).
Question 8.How many grams are there in:
i) 5 moles of water
ii) 2 moles of Ammonia
iii) 2 moles of Glucose
Answer:we know that in the case of compounds –
Molecular mass of water (H2O) = (2 + 16 ) = 18 grams
Molecular mass of ammonia (NH3) = ( 14+3) = 17 grams
Molecular mass of glucose ( C6H12O6) = ( 72 + 12+ 96) = 180 grams
Applying the above formula to all 3 cases-
(i) Mass = 5 x 18 = 90 grams
(ii) Mass = 2 x 17 = 34 grams
(iii) Mass = 2 x 180 = 360 grams
Modern atomic theory takes up the wave concept, principle of uncertainty and other latest discoveries to give a clear-cut picture about an atom. State the findings of modern atomic theory.
Answer:
● An atom is the smallest particle which takes part in chemical reaction.
● An atom is considered to be a divisible particle.
● The atoms of the same element may not be similar in all respects.
ex: Isotopes (17Cl35, 17Cl37 )
● The atoms of different elements may be similar in some respects.
ex. Isobars ( 18Ar40 , 20Ca40 )
● The ratio of atoms in a molecule may be fixed and integral but may not be simple. Ex.C12H22O11 is not a simple ratio. (Sucrose)
● The atoms of one element can be changed into the atoms of another element by transmutation.
● The mass of an atom can be converted into energy. This is in accordance with Einstein’s equation E = mc2 where E = energy, m = mass and c = velocity of light
Question 2.
How will you establish the relation between vapour density and molecular mass of a gas by applying Avogadro’s law?
Answer:
Relative Molecular Mass: It is defined as the ratio of the mass of 1 molecule of the gas or vapour to the mass of 1 atom of hydrogen.
Vapour Density (V.D): It is defined as the ratio of the mass of a certain volume of the gas or vapour to the mass of the same volume of hydrogen at the same temperature and pressure.
Applying Avogadro’s Law,
Since hydrogen is diatomic,
2 x V.D = relative molecular mass of a gas or vapour
2 x Vapour density = Relative molecular mass
Question 3.
Calculate the number of moles in:
i) 12.046 x 1023 atoms of Copper
ii) 27.95g of Iron
iii) 1.51 x 1023molecules of CO2
Answer:
we know that to find the number of moles, the following formulae are used:
(i) Using formula 3,
So, 2 moles of copper contain 12.046 x 1023 atoms of copper.
(ii) Using formula 1,
So, 0.5 moles consist of 27.95 grams of iron.
(iii) Using formula 4,
So, 0.25 moles of CO2 consists of 1.51 x 1023 molecules.
Note:
1. If a compound or molecular substance is taken, like CO2, N2 etc, then 1
a mole of the substance contains Avogadro number of molecules. 1 mole contains the mass equal to the molecular weight of the substance.
2. If an element is taken like C, S, Fe, then 1 mole contains Avogadro
number of atoms. 1 mole contains the mass equal to the atomic weight of the substance.
Question 4.
Find the gram molecular mass of the following from the data given:
i) H2O ii) CO2 iii) NaOH iv) NO2 v) H2SO4
Answer:
Molecular mass is the sum of the atomic masses of all the atoms present in one molecule of the substance.
1. H2O = (1gX2) + 16g = 18g
2. CO2 = 12g + (2 x16g) = 12 + 32 = 44g
3. NaOH = 23g + 16g + 1g = 40g
4. NO2 = 14 + (2 x 16) = 46g
5. H2SO4 = (1gx2) + 32g + (4x16g) = 98g
Question 5.
Complete the table given below:
Answer:
Formula used is
So, the complete table is
Question 6.
Calculate the number of water molecules present in one drop of water which weighs 0.18 g.
Answer:
According to mole concept we know that gram molecular weight of any compound consists of Avogadro number of molecules.
This implies that 18 grams of water consists 6.023 x 1023 molecules of water.
18 grams 6.023 x 1023 molecules
0.18 grams ?
Question 7.
Fill in the blanks using the given data:
The formula of Calcium oxide is CaO. The atomic mass of Ca is 40, Oxygen is 16 and Carbon is 12.
i) 1 mole of Ca ( ____g) and 1 mole of Oxygen atom ( ___g) combine to form _____mole of CaO ( ____g).
ii) 1 mole of Ca ( ___g) and 1 mole of C ( ___g) and 3 moles of Oxygen atom ( ___g) combine to form 1 mole of CaCO3 ( ___g)
Answer:
i) 1 mole of Ca ( 40 g) and 1 mole of an Oxygen atom ( 16 g) combine to form 1 mole of CaO ( 56 g).
ii) 1 mole of Ca ( 40 g) and 1 mole of C ( 12 g) and 3 moles of an Oxygen atom ( 3x16 = 48 g) combine to form 1 mole of CaCO3 ( 100 g)
Note:
1. If a compound or molecular substance is taken, like CO2, N2 etc, then 1
a mole of the substance contains Avogadro number of molecules. 1 mole contains the mass equal to the molecular weight of the substance.
2. If an element is taken like C, S, Fe, then 1 mole contains Avogadro
number of atoms. 1 mole contains the mass equal to the atomic weight of the substance.
So, 1 mole of Ca is 40 grams, 1 mole of O atom is 16 grams and 1 mole of C is 12 grams of C. 1 mole of CaO is 56 grams (40+16) of CaO and 1 mole of CaCO3 is 100 grams ( 40+12+48).
Question 8.
How many grams are there in:
i) 5 moles of water
ii) 2 moles of Ammonia
iii) 2 moles of Glucose
Answer:
we know that in the case of compounds –
Molecular mass of water (H2O) = (2 + 16 ) = 18 grams
Molecular mass of ammonia (NH3) = ( 14+3) = 17 grams
Molecular mass of glucose ( C6H12O6) = ( 72 + 12+ 96) = 180 grams
Applying the above formula to all 3 cases-
(i) Mass = 5 x 18 = 90 grams
(ii) Mass = 2 x 17 = 34 grams
(iii) Mass = 2 x 180 = 360 grams
Part-c
Question 1.When ammonia reacts with hydrogen chloride gas, it produces white fumes of ammonium chloride. The volume occupied by NH3 in glass bulb A is three times more than the volume occupied by HCl in glass bulb B at STP.
i) How many moles of ammonia are present in glass bulb A?
ii) How many grams of NH4Cl will be formed when the stopper is opened?
(Atomic mass of N = 14, H = 1, Cl = 35.5)
iii) Which gas will remain after completion of the reaction?
iv) Write the chemical reaction involved in this process.
Answer:(i) 3 moles
(ii) 53.5 grams (14 + 4 + 35.5)
(iii) Ammonia ( 2 moles will be remaining )
(iv) NH3 + HCl 
NH4Cl
Explanation -1 mole of any gas at STP occupies 22.4 litres of volume. So, 1 mole of ammonia occupies 22.4 litres of volume. 67.2 litres (22.4 x 3) of volume is 3 moles of ammonia. 22.4 litres of HCl is 1 mole of HCl. According to reaction ,1 mole of ammonia reacts with 1 mole of HCl to form 1 mole of NH4Cl, which comes out as white fumes.
NH3 + HCl NH4Cl
Even though 3 moles of ammonia is present in bulb, only one 1 mole undergoes reaction with 1 mole of HCl. The other 2 moles of ammonia remain unreacted.
Question 2.Nitro glycerine is used as an explosive. The equation for the explosive reaction is
4C3H5((NO3))312CO2 + 10H2O + 6N2 + O2
(l) (g) (l) (g) (g)
(Atomic mass of C = 12, H = 1, N = 14, O=16)
1. How many moles does the equation show for i) Nitroglycerine ii) gas molecules produced?
2. How many moles of gas molecules are obtained from 1 mole of nitroglycerine?
3. What is the mass of 1 mole of nitroglycerine?
Answer:1. 4 moles of nitroglycerine ; CO2 (12) + N2(6) + O2(1) = 19 moles of
gas molecules are formed.
2. 4 moles of nitroglycerine gives 19 moles of gas molecules. So, 1 mole
of nitroglycerine gives (19/4) 4.75 moles of gas molecules.
3. Gram molecular mass of nitroglycerine is 1 mole of nitroglycerine.
So, mass of 1 mole of nitroglycerine is 227 grams.
[(3x12)C + (5x1)H + (3x14)N + (9x16)O]
Question 3.Sodium bi carbonate breaks down on heating:
2NaHCO3 Na2CO3 + H2O + CO2
(Atomic mass of Na = 23, C = 12, H = 1, O=16)
i) How many moles of sodium bi carbonate are there in the equation?
ii) What is the mass of sodium bicarbonate used in this equation?
iii) How many moles of carbon dioxide are there in this equation?
Answer:(i) Two (coefficient of sodium bi carbonate)
(ii) 1 mole of sodium bi carbonate contains 84 grams. Two moles of
sodium bi carbonate contains 168 grams. So, 168 grams of sodium bi carbonate is used in the equation.
(iii) 1 mole (coefficient of CO2 )
Question 4.40 g of calcium was extracted from 56 g of calcium oxide
(Atomic mass of Ca= 40, O=16)
i) What mass of oxygen is there in 56 g of calcium oxide?
ii) How many moles of oxygen atoms are there in this?
iii) How many moles of calcium atoms are there in 40 g of calcium?
iv) What mass of calcium will be obtained from 1000 g of calcium oxide?
Answer:(i) 16 grams of O
(ii) 1 mole of oxygen atoms
(iii) 1 mole
(iv) 714.38 grams.
56 grams of CaO gives 40 grams of Ca. 1000 grams of CaO gives (1000x40)/56 = 714.28 grams of calcium
Explanation –
CaO 
Ca + O
56 40 16
1 mole of any compound (or gas in molecular form) contains the mass equal to its gram molecular mass. 1 mole of any element contains the mass equal to its gram atomic mass. So,
1 mole of CaO = 40 + 16 = 56 grams
1 mole of Ca = 40 grams
1 mole of oxygen atoms = 16 grams
1 mole of calcium oxide dissociates to form 1 mole of Ca and 1 mole of O atoms.
Question 5.How many grams are there in the following?
i) 1 mole of chlorine molecule, Cl2
ii) 2 moles of sulphur molecules, S8
iii) 4 moles of ozone molecules, O3
iv) 2 moles of nitrogen molecules, N2
Answer:we know that when gases are present in the molecular form, 1 mole of any gas is equal to 6.023 x 1023 molecules of that gas, which is equal to the gram molecular weight of gas in the combined state.
(i) 1 mole of chlorine molecules contains 71 grams of Cl2. (2×35.5)
(ii) 2 moles of sulphur molecules contain 512 grams of S8. (2×32×8)
(iii) 4 moles of ozone molecules contain 192 grams of O3. (4× 16× 3)
(iv) 2 moles of nitrogen molecules contain 56 grams of N2. (2× 14× 2)
Question 6.Find how many moles of atoms are there in:
i) 2 g of nitrogen.
ii) 23 g of sodium
iii) 40 g of calcium.
iv) 1.4 g of lithium
v) 32 g of sulphur.
Answer:
We know the formula that
Applying the above formula for all cases.
(i) 
(ii) 
(iii) 
(iv) 
(v) 
When ammonia reacts with hydrogen chloride gas, it produces white fumes of ammonium chloride. The volume occupied by NH3 in glass bulb A is three times more than the volume occupied by HCl in glass bulb B at STP.
i) How many moles of ammonia are present in glass bulb A?
ii) How many grams of NH4Cl will be formed when the stopper is opened?
(Atomic mass of N = 14, H = 1, Cl = 35.5)
iii) Which gas will remain after completion of the reaction?
iv) Write the chemical reaction involved in this process.
Answer:
(i) 3 moles
(ii) 53.5 grams (14 + 4 + 35.5)
(iii) Ammonia ( 2 moles will be remaining )
(iv) NH3 + HCl NH4Cl
Explanation -1 mole of any gas at STP occupies 22.4 litres of volume. So, 1 mole of ammonia occupies 22.4 litres of volume. 67.2 litres (22.4 x 3) of volume is 3 moles of ammonia. 22.4 litres of HCl is 1 mole of HCl. According to reaction ,1 mole of ammonia reacts with 1 mole of HCl to form 1 mole of NH4Cl, which comes out as white fumes.
NH3 + HCl NH4Cl
Even though 3 moles of ammonia is present in bulb, only one 1 mole undergoes reaction with 1 mole of HCl. The other 2 moles of ammonia remain unreacted.
Question 2.
Nitro glycerine is used as an explosive. The equation for the explosive reaction is
4C3H5((NO3))312CO2 + 10H2O + 6N2 + O2
(l) (g) (l) (g) (g)
(Atomic mass of C = 12, H = 1, N = 14, O=16)
1. How many moles does the equation show for i) Nitroglycerine ii) gas molecules produced?
2. How many moles of gas molecules are obtained from 1 mole of nitroglycerine?
3. What is the mass of 1 mole of nitroglycerine?
Answer:
1. 4 moles of nitroglycerine ; CO2 (12) + N2(6) + O2(1) = 19 moles of
gas molecules are formed.
2. 4 moles of nitroglycerine gives 19 moles of gas molecules. So, 1 mole
of nitroglycerine gives (19/4) 4.75 moles of gas molecules.
3. Gram molecular mass of nitroglycerine is 1 mole of nitroglycerine.
So, mass of 1 mole of nitroglycerine is 227 grams.
[(3x12)C + (5x1)H + (3x14)N + (9x16)O]
Question 3.
Sodium bi carbonate breaks down on heating:
2NaHCO3 Na2CO3 + H2O + CO2
(Atomic mass of Na = 23, C = 12, H = 1, O=16)
i) How many moles of sodium bi carbonate are there in the equation?
ii) What is the mass of sodium bicarbonate used in this equation?
iii) How many moles of carbon dioxide are there in this equation?
Answer:
(i) Two (coefficient of sodium bi carbonate)
(ii) 1 mole of sodium bi carbonate contains 84 grams. Two moles of
sodium bi carbonate contains 168 grams. So, 168 grams of sodium bi carbonate is used in the equation.
(iii) 1 mole (coefficient of CO2 )
Question 4.
40 g of calcium was extracted from 56 g of calcium oxide
(Atomic mass of Ca= 40, O=16)
i) What mass of oxygen is there in 56 g of calcium oxide?
ii) How many moles of oxygen atoms are there in this?
iii) How many moles of calcium atoms are there in 40 g of calcium?
iv) What mass of calcium will be obtained from 1000 g of calcium oxide?
Answer:
(i) 16 grams of O
(ii) 1 mole of oxygen atoms
(iii) 1 mole
(iv) 714.38 grams.
56 grams of CaO gives 40 grams of Ca. 1000 grams of CaO gives (1000x40)/56 = 714.28 grams of calcium
Explanation –
CaO Ca + O
56 40 16
1 mole of any compound (or gas in molecular form) contains the mass equal to its gram molecular mass. 1 mole of any element contains the mass equal to its gram atomic mass. So,
1 mole of CaO = 40 + 16 = 56 grams
1 mole of Ca = 40 grams
1 mole of oxygen atoms = 16 grams
1 mole of calcium oxide dissociates to form 1 mole of Ca and 1 mole of O atoms.
Question 5.
How many grams are there in the following?
i) 1 mole of chlorine molecule, Cl2
ii) 2 moles of sulphur molecules, S8
iii) 4 moles of ozone molecules, O3
iv) 2 moles of nitrogen molecules, N2
Answer:
we know that when gases are present in the molecular form, 1 mole of any gas is equal to 6.023 x 1023 molecules of that gas, which is equal to the gram molecular weight of gas in the combined state.
(i) 1 mole of chlorine molecules contains 71 grams of Cl2. (2×35.5)
(ii) 2 moles of sulphur molecules contain 512 grams of S8. (2×32×8)
(iii) 4 moles of ozone molecules contain 192 grams of O3. (4× 16× 3)
(iv) 2 moles of nitrogen molecules contain 56 grams of N2. (2× 14× 2)
Question 6.
Find how many moles of atoms are there in:
i) 2 g of nitrogen.
ii) 23 g of sodium
iii) 40 g of calcium.
iv) 1.4 g of lithium
v) 32 g of sulphur.
Answer:
We know the formula that
Applying the above formula for all cases.
(i)
(ii)
(iii)
(iv)
(v)
