Class 9 is the first stepping stone for a student in the competitive world. With the introduction of the CBSE Board Exam for class 10 a few years back, this has become an important gateway for a student. Based on the results of class 9th a student selects his future stream of Science, Commerce or Arts suiting his interest.
Takshila Learning is providing NCERT Solutions for Class 9 Science as per the latest syllabus by CBSE. Class 9 is the building block for the CBSE Class 10 Board Exams, not only for your exams but also for your higher studies and career. Science is the most essential subject and the knowledge in this field opens up wider career opportunities for the students.
Below you can find the NCERT solution for Class 9th Science. You can get a Solution for the all-important question of “Atoms and Molecules”
Intext questions (set 1)
QUES 1: In a reaction, 5.3g of sodium carbonate reacted with 6 g of acetic acid. The products were 2.2 g of carbon dioxide, 0.9 g water and 8.2 g of sodium acetate. Show that these observations are in agreement with the law of conservation of mass.
As per the law of conservation of mass, the total mass of reactants must be equal to the total mass of
As per the above reaction, LHS = RHS i.e., 5.3g + 6g = 2.2g + 0.9 g + 8.2 g = 11.3 g
Hence the observations are in agreement with the law of conservation of mass.
Ques 2: Hydrogen and oxygen combine in the ratio of 1:8 by mass to form water. What mass of oxygen gas would be required to react completely with 3 g of hydrogen gas?
We know hydrogen and water mix in the ratio 1: 8.
For every 1g of hydrogen, it is 8g of oxygen.
Therefore, for 3g of hydrogen, the quantity of oxygen = 3 x 8 = 24g
Hence, 24g of oxygen would be required for the complete reaction with 3g of hydrogen gas.
Ques 3: Which postulate of Dalton’s atomic theory is the result of the law of conservation of mass?
The postulate of Dalton’s Atomic theory which is a result of the law of conservation of mass is, “Atoms can neither be created nor destroyed”.
Ques 4: Which postulate of Dalton’s atomic theory can explain the law of definite proportions?
Answer: The postulate of Dalton’s atomic theory that can explain the law of definite proportions is – the relative number and kinds of atoms are equal in given compounds.
Intext questions (set 2)
Ques 1: Define the atomic mass unit?
Answer: An atomic mass unit is a unit of mass used to express weights of atoms and molecules where one atomic mass is equal to 1/12th the mass of one carbon-12 atom.
Ques 2: Why is it not possible to see an atom with naked eyes?
Answer: The size of atom is so small that it is not possible to see it with naked eyes. Also, the atom of an element does not exist independently.
Intext questions (set 3)
Page no. 39
Ques 1: Write down the formulae of
(i) sodium oxide
(ii) aluminium chloride
(iii) sodium sulphide
(iv) magnesium hydroxide
The following are the formulae:
(i) sodium oxide – Na2O
(ii) aluminium chloride – AlCl3
(iii) sodium sulphide – Na2S
(iv) magnesium hydroxide – Mg (OH)2
Ques 2: Write down the names of compounds represented by the following formulae:
Listed below are the names of the compounds for each of the following formulae
(i) Al2(SO4)3 – Aluminium sulphate
(ii) CaCl2 – Calcium chloride
(iii) K2SO4 – Potassium sulphate
(iv) KNO3 – Potassium nitrate
(v) CaCO3 – Calcium carbonate.
Ques 3: What is meant by the term chemical formula?
Answer: Chemical formula is the symbolic representation of a chemical compound. For example: The chemical formula of hydrochloric acid is HCl.
Ques 4: How many atoms are present in a
(i) H2S molecule and
(ii) PO43- ion?
Answer: The number of atoms present are as follows:
(i) H2S molecule has 2 atoms of hydrogen and 1 atom of sulphur hence 3 atoms in totality.
(ii) PO43- ion has 1 atom of phosphorus and 4 atoms of oxygen hence 5 atoms in totality.
Ques 1: Calculate the molecular masses of H2 , O2 , Cl2, CO2, CH4, C2H6, C2H4, NH3, CH3OH.
Answer: The following are the molecular masses:
- molecular mass of H2– 2 x atoms atomic mass of H = 2 x 1u = 2u
- molecular mass of O2– 2 x atoms atomic mass of O = 2 x 16u = 32u
- molecular mass of Cl2– 2 x atoms atomic mass of Cl = 2 x 35.5u = 71u
- molecular mass of CO2– atomic mass of C + 2 x atomic mass of O = 12 + ( 2×16)u = 44u
- molecular mass of CH4– atomic mass of C + 4 x atomic mass of H = 12 + ( 4 x 1)u = 16u
- molecular mass of C2H6– 2 x atomic mass of C + 6 x atomic mass of H = (2 x 12) +(6 x 1)u=24+6=30u
- molecular mass of C2H4– 2 x atomic mass of C + 4 x atomic mass of H = (2x 12) +(4 x 1)u=24+4=28u
- molecular mass of NH3– atomic mass of N + 3 x atomic mass of H = (14 +3 x 1)u= 17u
- molecular mass of CH3OH – atomic mass of C + 3x atomic mass of H + atomic mass of O + atomic mass of H = (12 + 3×1+16+1)u=(12+3+17)u = 32u
Ques 2: Calculate the formula unit masses of ZnO, Na2O, K2CO3, given atomic masses of Zn = 65u, Na = 23 u, K=39u, C = 12u, and O=16u.
Atomic mass of Zn = 65u
Atomic mass of Na = 23u
Atomic mass of K = 39u
Atomic mass of C = 12u
Atomic mass of O = 16u
The formula unit mass of ZnO= Atomic mass of Zn + Atomic mass of O = 65u+16u = 81u
The formula unit mass of Na2O = 2 x Atomic mass of Na + Atomic mass of O = (2 x 23)u +16u=46u+16u=62u
Intext questions (set 5)
Ques 1: If one mole of carbon atoms weighs 12grams, what is the mass (in grams) of 1 atom of carbon?
Answer: Given: 1 mole of carbon weighs 12g
1 mole of carbon atoms = 6.022 X 1023
Molecular mass of carbon atoms = 12g = an atom of carbon mass
Hence, mass of 1 carbon atom = 12 / 6.022 X 1023 = 1.99 X 10-23g
Ques 2: Which has more number of atoms, 100 grams of sodium or 100 grams of iron (given, atomic mass of Na = 23u, Fe = 56 u)?
Answer: Given: Atomic mass of Na=23u, Atomic mass of Fe= 56u
To calculate the number of atoms in 100g of sodium:
23g of Na contains = 6.022 X 1023 atoms
1g of Na contains = 6.022 X 1023 atoms / 23
100g of Na contains = 6.022 X 1023 atoms X 100 / 23
= 2.6182 X 1024 atoms
To calculate the number of atoms in 100g of sodium:
56g of Fe contains = 6.022 X 1023 atoms
1g of Fe contains = 6.022 X 1023 atoms / 56
100g of Fe contains = 6.022 X 1023 atoms X 100 / 56
= 1.075 X 1024 atoms
Hence, through comparison, it is evident that 100g of Na has more atoms.
Q1. A 0.24g sample of compound of oxygen and boron was found by analysis to contain 0.096g of boron and 0.144g of oxygen. Calculate the percentage composition of the compound by weight.
Answer: Given: Mass of the sample compound = 0.24g, mass of boron = 0.096g, mass of oxygen = 0.144g
To calculate percentage composition of the compound:
Percentage of boron = mass of boron / mass of the compound x 100
= 0.096g / 0.24g x 100 = 40%
Percentage of oxygen = 100 – percentage of boron
= 100 – 40 = 60%
Q2. When 3.0g of carbon is burnt in 8.00 g of oxygen, 11.00 g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combination will govern your answer?
Answer: 11.00g of carbon dioxide is formed when 3.00g carbon is burnt in 8.00g of oxygen.
Carbon and oxygen are combined in the ratio 3:8 to give carbon dioxide using up all the carbon and
Hence, for 3g of carbon and 50g of oxygen, 8g of oxygen is used and 11g of carbon is formed, the
left oxygen is unused i.e., 50-3=47g of oxygen is unused.
This depicts the law of definite proportions – The combining elements in compounds are present in
definite proportions by mass.
Q3. What are polyatomic ions? Give examples.
Answer: Polyatomic ions are ions that contain more than one atom but they behave as a single unit
Example: CO32- , H2PO4–
Q4. Write the chemical formula of the following.
(a) Magnesium chloride
(b) Calcium oxide
(c) Copper nitrate
(d) Aluminium chloride
(e) Calcium carbonate
Answer: The following are the chemical formula of the above-mentioned list:
(a) Magnesium chloride – MgCl2
(b) Calcium oxide – CaO
(c) Copper nitrate – Cu(NO3)2
(d) Aluminium chloride – AlCl3
(e) Calcium carbonate – CaCO3
Q5. Give the names of the elements present in the following compounds.
(a) Quick lime
(b) Hydrogen bromide
(c) Baking powder
(d) Potassium sulphate.
Answer: The following are the names of the elements present in the following compounds:
(a) Quick lime – Calcium and oxygen (CaO)
(b) Hydrogen bromide – Hydrogen and bromine (HBr)
(c) Baking powder – Sodium, Carbon, Hydrogen, Oxygen (NaHCO3)
(d) Potassium sulphate – Sulphur, Oxygen, Potassium (K2SO4)
Q6. Calculate the molar mass of the following substances.
(a) Ethyne, C2H2
(b) Sulphur molecule, S8
(c) Phosphorus molecule, P4 (Atomic mass of phosphorus =31)
(d) Hydrochloric acid, HCl
(e) Nitric acid, HNO3
Listed below is the molar mass of the following substances:
(a) Molar mass of Ethyne C2H2= 2 x Mass of C+2 x Mass of H = (2×12)+(2×1)=24+2=26g
(b) Molar mass of Sulphur molecule S8 = 8 x Mass of S = 8 x 32 = 256g
(c) Molar mass of Phosphorus molecule, P4 = 4 x Mass of P = 4 x 31 = 124g
(d) Molar mass of Hydrochloric acid, HCl = Mass of H+ Mass of Cl = 1+35.5 = 36.5g
(e) Molar mass of Nitric acid, HNO3 =Mass of H+ Mass of Nitrogen + 3 x Mass of O = 1 + 14+
3×16 = 63g
Q7. What is the mass of –
(a) 1 mole of nitrogen atoms?
(b) 4 moles of aluminium atoms((Atomic mass of aluminium =27)?
(c) 10 moles of sodium sulphite (Na2SO3)?
Answer: The mass of the above mentioned list is as follows:
(a) Atomic mass of nitrogen atoms = 14u
Mass of 1 mole of nitrogen atoms= Atomic mass of nitrogen atoms
Therefore, mass of 1 mole of nitrogen atom is 14g
(b) Atomic mass of aluminium =27u
Mass of 1 mole of aluminium atoms = 27g
1 mole of aluminium atoms = 27g, 4 moles of aluminium atoms = 4 x 27 = 108g
(c) Mass of 1 mole of sodium sulphite Na2SO3 = Molecular mass of sodium sulphite = 2 x Mass of Na + Mass of S + 3 x Mass of O = (2 x 23) + 32 +(3x 16) = 46+32+48 = 126g
Therefore, mass of 10 moles of Na2SO3 = 10 x 126 = 1260g
Q8. Convert into mole.
(a) 12g of oxygen gas
(b) 20g of water
(c) 22g of carbon dioxide
Answer: Conversion of the above-mentioned molecules into moles is as follows:
(a) Given: Mass of oxygen gas=12g
Molar mass of oxygen gas = 2 Mass of Oxygen = 2 x 16 = 32g
Number of moles = Mass given / molar mass of oxygen gas = 12/32 = 0.375 moles
(b) Given: Mass of water = 20g
Molar mass of water = 2 x Mass of Hydrogen + Mass of Oxygen = 2 x 1 + 16 = 18g
Number of moles = Mass given / molar mass of water
= 20/18 = 1.11 moles
(c) Given: Mass of carbon dioxide = 22g
Molar mass of carbon dioxide = Mass of C + 2 x Mass of Oxygen = 12 + 2x 16 = 12+32=44g
Number of moles = Mass given/ molar mass of carbon dioxide = 22/44 = 0.5 moles
Q9. What is the mass of:
(a) 0.2 mole of oxygen atoms?
(b) 0.5 mole of water molecules?
Answer: The mass is as follows:
(a) Mass of 1 mole of oxygen atoms = 16u, hence it weighs 16g
Mass of 0.2 moles of oxygen atoms = 0.2 x 16 = 3.2u
(b) Mass of 1 mole of water molecules = 18u, hence it weighs 18g
Mass of 0.5 moles of water molecules = 0.5 x 18 = 9u
Q10. Calculate the number of molecules of sulphur (S8) present in 16g of solid sulphur.
Answer: To calculate molecular mass of sulphur:
Molecular mass of Sulphur (S8) = 8xMass of Sulphur = 8×32 = 256g
Mass given = 16g
Number of moles = mass given/ molar mass of sulphur
= 16/256 = 0.0625 moles
To calculate the number of molecules of sulphur in 16g of solid sulphur:
Number of molecules = Number of moles x Avogadro number
= 0.0625 x 6.022 x 10²³ molecules
= 3.763 x 1022 molecules
Q11. Calculate the number of aluminium ions present in 0.051g of aluminium oxide.
(Hint: The mass of an ion is the same as that of an atom of the same element. Atomic mass of Al = 27u)
Answer: To calculate the number of aluminium ions in 0.051g of aluminium oxide:
1 mole of aluminium oxide = 6.022 x 1023 molecules of aluminium oxide
1 mole of aluminium oxide (Al2O3) = 2 x Mass of aluminium + 3 x Mass of Oxygen
= (2x 27) + (3 x16) = 54 +48 = 102g
1 mole of aluminium oxide = 102g = 6.022 x 1023 molecules of aluminium oxide
Therefore, 0.051g of aluminium oxide has = 0.051 x 6.022 x 1023 / 102
= 3.011 x 1020 molecules of aluminium oxide
One molecule of aluminium oxide has 2 aluminium ions, hence number of aluminium ions present in 0.051g of aluminium oxide = 2 x 3.011x 1020 molecules of aluminium oxide
= 6.022 x 1020
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