# Atoms and Molecules Questions and Answers Class 9

## Atoms and Molecules Class 9 Questions and Answers

Page-32

Q1. In a reaction 5.3 g of sodium carbonate reacted with 6 g of ethanoic acid. The products were 2.2 g of carbon dioxide, 0.9g water and 8.2 g of sodium ethanoate. Show that these observations are in agreement with the law of conservation of mass.

Sodium carbonate + ethanoic acid → sodium ethanoate + carbon dioxide + water.

Solution: In a reaction, Sodium carbonate reacts with ethanoic acid to produce Sodium ethanoate, Carbon dioxide, and water.

Sodium     +      Ethanoic → Sodium  +     Carbon  +    Water

Carbonate          acid             ethanoate       dioxide

Mass of sodium carbonate = 5.3g (Given)

Mass of ethanoic acid = 6g (Given)

Mass of sodium ethanoate = 8.2g (Given)

Mass of carbon dioxide = 2.2 (Given)

Mass of water = 0.9g    (Given)

Now, total mass before the reaction = (5.3 + 6)g

= 11. 3g

and total mass after the reaction = (8.2 + 2.2 + 0.9)g = 11.3g

Therefore, Total mass before the reaction = Total mass after the reaction

Hence, the given observations are in agreement with the law of conservation of mass.

Page-33

Q2. 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 3g of hydrogen gas?

Solution: It is given that the ratio of hydrogen and oxygen by mass to form water is 1:8. Then, the mass of oxygen gas required to react completely with 1g of hydrogen gas is 8g. Therefore, the mass of oxygen gas required to react completely with 3g of hydrogen gas is 8 × 3g = 24 g.

Q3. Which postulate of Dalton’s atomic theory is the result of the law of conservation of mass?

Solution: The postulate of Dalton’s atomic theory which is a result of the law of conservation of mass is “Atoms are indivisible particles, which can neither be created nor destroyed in a chemical reaction”.

Q4. Which postulate of Dalton’s atomic theory can explain the law of definite proportions?

Solution: The postulate of Dalton’s atomic theory which can explain the law of definite proportion is “The relative number and kind of atoms in a given compound remain constant”.

Page-35

Q1. Define atomic mass unit.

Solution: Mass unit equal to exactly one-twelfth the mass of one atom of carbon – 12 is called one atomic mass unit. It is written as ‘u’.

Q2. Why is it not possible to see an atom with naked eyes?

Solution: The size of an 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.

Page-39

Q1. Write down the formula of

Solution:

Q2. Write down the names of compounds represented by the following formula:

• Al2(SO4)3
• CaCl2
• K2SO4
• KNO3
• CaCO3

Solution:

• Al(SO4)3→ Aluminium sulphate
• CaCl2→ Calcium chloride
• K2SO4→ Potassium sulphate
• CaCO3→ Calcium carbonate

Q3. What is meant by the term chemical formula?

Solution: The chemical formula of a compound means the symbolic representation of the composition of a compound. From the chemical formula of a compound, we can know the number and kinds of atoms of different elements that constitute the compound. For example, from the chemical formula CO2 of carbon dioxide, we come to know that one carbon atom and two oxygen atoms are chemically bonded together to form one molecule of the compound, carbon dioxide.

Q4. How many atoms are present in a :

1. H2S molecule and

2. PO4 3-ion?

Solution:

1. In an H2S molecule, three atoms are present; two of hydrogen and one of Sulphur.

2. In a PO4 3-  ion, five atoms are present; one of phosphorus and four of oxygen.

Page-40

Q1. Calculate the molecular masses of H2, O2, Cl2, CO2, CH4, C2H6, C2H4, NH3, CH3OH.

Solution:

Molecular mass of H2= 2 × Atomic mass of H

Molecular mass of Cl2= 2 × Atomic mass of Cl

= 2 × 35.5 = 71 u

Molecular mass of CO2= Atomic mass of C + 2 × Atomic mass of O

Molecular mass of C2H6= 2 × Atomic mass of C + 6 × Atomic mass of H = 2 × 12 + 6 × 1 = 30u

Molecular mass of C2H4= 2 × Atomic mass of C + 4 × Atomic mass of H = 2 × 12 + 4 × 1 = 28u

Molecular mass of NH3= Atomic mass of N + 3 × Atomic mass of H = 14 + 3 × 1 =17 u

Molecular mass of CH3OH Atomic mass of C+4 ×Atomic mass of H+Atomic mass of O = 12 + 4 × 1 + 16 = 32 u

Q2. Calculate the formula unit masses of ZnO, Na2O, K2CO3, given masses of Zn = 65u, Na = 23u, K = 39u, C = 12u, and O = 16u.

Solution: Formula unit mass of ZnO = Atomic mass of Zn + Atomic mass of O = 65 + 16 = 81 u

Formula unit mass of Na2O = 2 × Atomic mass of Na + Atomic mass of O = 2 × 23 + 16 = 62u

Formula unit mass of K2CO3

=> 2 × Atomic mass of K + Atomic mass of C + 3 × Atomic mass of O

=> 2 × 39 + 12 + 3 × 16  = 138u

Page-42

Q1. If one mole of carbon atoms weighs 12 grams, what is the mass (in gram) of 1 atom of carbon?

Solution: One mole of carbon atoms weighs 12g (Given)

i.e., the mass of 1 mole of carbon atoms = 12g

Then, the mass of 6.022× 1023 number of carbon atoms = 12g

Therefore, the mass of 1 atom of carbon

=6.022×1023g = 1.9926 × 1023g

Q2. Which has more number of atoms, 100 grams of sodium or 100 grams of iron (given, the atomic mass of Na = 23u, Fe =56 u)?

Solution:

It is given

Atomic mass of Na = 23u

Then, gram atomic mass of Na = 23g

Now, 23g of Na contains = 6.022×1023number of atoms

Thus, 100g of Na contains

Then, 1 gram atomic mass of Fe = 56g

Now, 56 g of Fe contains = 6.022×1023number of atoms

= 1.0753 × 1024number of atoms

Therefore, 100 grams of sodium contain more number of atoms than 100 grams of iron.

Exercise

Q1. A 0.24 g sample of a compound of oxygen and boron was found by analysis to contain 0.096 g if boron and 0.144 g of oxygen. Calculate the percentage composition of the compound by weight.

Solution:

Mass of boron = 0.096g

Mass of oxygen = 0.144g

Mass of sample = 0.24g

Thus, percentage of boron by weight in the compound =

= 40%

Thus, percentage of oxygen by weight in the compound =

Q2. When 3.0 g of carbon is burnt in 8.00 g oxygen, 11.00 g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00 g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combinations will govern your answer?

Solution:  Carbon + Oxygen → Carbon dioxide

3g of carbon reacts with 8 g of oxygen to produce 11g of carbon dioxide. If 3g of carbon is burnt in 50g of oxygen, then 3g of carbon will react with 8 g of oxygen. The remaining 42 g of oxygen will be left un-reactive. In this case, also, only 11g of carbon dioxide will be formed. The above answer is governed by the law of constant proportions.

Q3. What are polyatomic ions? Give examples?

Solution: A polyatomic ion is a group of atoms carrying a charge (positive or negative).

For example, ammonium ion (Al4+), hydroxide ion (OH), carbonate ion ( CO32−).

Q4. Write the chemical formula of the following:

1. Magnesium chloride

2. Calcium oxide

3. Copper nitrate

4. Aluminium chloride

5. Calcium carbonate

Solution:

1. Magnesium chloride →MgCl2

2. Calcium oxide →CaO

3. Copper nitrate →Cu(NO3)2

4. Aluminium chloride →AlCl3

5. Calcium carbonate →CaCO3

Q5. Give the names of the elements present in the following compounds:

Quick lime

Hydrogen bromide

Baking powder

Potassium sulphate.

Solution:

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

Solution:

Q7. What is the mass of:

1. 1 mole of nitrogen atoms?

2. 4 mole of Aluminium atoms (Atomic mass of Aluminium = 27)?

3. 10 moles of sodium Sulphite (Na2SO3)?

Solution:

1. The mass of 1 mole of nitrogen atoms is 14g.

2. The mass of 4 moles of Aluminium atoms is (4 × 27)g = 108g

3. The mass of 10 moles of sodium Sulphite (Na2SO3) is

=> 10 × [2 × 23 + 32 + 3 × 16]g

=> 10 × 126g = 1260g

Q8. Convert into mole:

(a). 12g of oxygen gas

(b). 12g of water

(c). 22g of carbon dioxide

Solution:32 g of oxygen gas = 1 mole

(a) 32 g of oxygen gas = 1 mole
12 g of oxygen gas = 12/32 = 0.375 mole

(b) 18g of water = 1 mole

Then, 20 g of water = 20/18 mole = 1.11 moles (approx.)44g of carbon dioxide = 1 mole

(c) 44g of carbon dioxide = 1 mole

Then, 22g of carbon dioxide = 22/44 mole = 0.5 mole

Q9. What is the mass of:0.2 mole of oxygen atoms?

(a). 0.2 mole of oxygen atoms?

(b). 0.5 mole of water molecules?

Solution:Mass of one mole of oxygen atoms = 16g

(a) Mass of one mole of oxygen atoms = 16g

Then, mass of 0.2 mole of oxygen atoms = 0.2 × 16g = 3.2gMass of one mole of water molecule = 18g

(b) Mass of one mole of water molecule = 18g

Then, mass of 0.5 mole of water molecules = 0.5 × 18g = 9g

Q10. Calculate the number of molecules of sulphur (S8) present in 16g of solid sulphur.

Solution: 1 mole of solid sulphur (S8) = 8 × 32g = 256g

i.e., 256g of solid sulphur contains = 6.022 × 1023molecules

Then, 16g of solid sulpur contains 6.022 × 1023× 16molecules

= 3.76 × 1022molecules (approx)

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)

Solution: 1 mole of aluminium oxide (Al2O3) = 2 × 27 + 3 × 16 = 102g

i.e., 102g of Al2O3= 6.022 × 1023molecules of Al2O3

= 3.011 × 1020  molecules of Al2O3

The number of aluminium ions (Al3+) present in one molecules of aluminium oxide is 2. Therefore, The number of aluminium ions (Al3+) present in

3.11 × 1020molecules (0.051g) of aluminium oxide (Al2O3) = 2 × 3.011 × 1020= 6.022 × 1020

Try To Solve These Questions

Q1. What is 1 amu?

Q2. What is Law of definite proportions.

Q3. Define Valency.

### 4 thoughts on “Atoms and Molecules Questions and Answers Class 9”

1. good post