Model Test Questions Class 9 Chemistry Test #4 for Chapter # 1 (Fundamentals of Chemistry)|Updated 2026-27 (SLO)

 

📘 Model Test Questions Class 9 Chemistry
Test # 4 for Chapter # 2
(Fundamentals of Chemistry)

amu, molar mass, atomic mass, Avogadro’s number, mole, average atomic mass, molecular mass, formula mass, gram atomic mass, gram molecular mass, gram formula mass, molar volume
Numericals on mole concept and Balancing of equations

👨‍🏫 Prepared by Inam Jazbi – Learn Chemistry

This model test paper is designed according to the latest examination pattern. Students should prepare the following important topics carefully.

• 🧪 Atomic, molecular and formula mass
• 📊 Gram atomic, molecular and formula mass
• ⚖️ Mole and Avogadro’s number
• 🧂 molar mass
• 🏭 molar volume
• 💡 Numericals on mole concept
• 🔬 Balancing of equations

📘 Short Answer Questions (SLO Based)

👨‍🏫 Prepared by Inam Jazbi – Learn Chemistry

Q1.

Define amu, molar mass, atomic mass, Avogadro’s number, mole, average atomic mass, molecular mass, formula mass, gram atomic mass, gram molecular mass, gram formula mass and molar volume.

Q2.

Write down the differences between the following: (i) Atomic mass and Molecular mass. (ii) Molecular mass and Formula mass.

Q3.

What is chemical formula? Describe the relationship between empirical formula and molecular formula with suitable examples.

Complete the following chart:

Compound	Molecular Formula	Integer (n)	Empirical Formula
Ethene	C2H4
Hydrogen peroxide	H2O2
Glucose	C6H12O6

Q4.

Write down the chemical formula, empirical formula and molecular formula of the following compounds: • Sulphuric acid • Carbon dioxide • Glucose • Benzene • Ethene • Ethyne • Hydrogen peroxide • Acetic acid

Q5.

Differentiate between empirical formula and molecular formula. Find the molecular formula of a compound if its empirical formula is CH₂O and its molecular mass is 60 amu.

Q6.

Complete and balance the following chemical equations:
1. 2KClO₃ → 2KCl + 3O₂
2. 2KNO₃ → 2KNO₂ + O₂
3. 2Ba(NO₃)₂ → 2BaO + 4NO₂ + O₂
4. 2FeSO₄ → Fe₂O₃ + SO₂ + SO₃
5. 2Na + 2H₂O → 2NaOH + H₂
6. 2NH₃ + 3Cl₂ → N₂ + 6HCl
7. 3CuO + 2NH₃ → 3Cu + N₂ + 3H₂O
8. MnO₂ + 4HCl → MnCl₂ + 2H₂O + Cl₂
9. 4NH₃ + 5O₂ → 4NO + 6H₂O
10. 4NH₃ + 7O₂ → 4NO₂ + 6H₂O
11. PCl₃ + 3H₂O → 3HCl + H₃PO₃
12. Cu + 2H₂SO₄ → CuSO₄ + SO₂ + 2H₂O
13. 4Zn + 10HNO₃ → 4Zn(NO₃)₂ + NH₄NO₃ + 3H₂O

📘 Numericals

👨‍🏫 Prepared by Inam Jazbi – Learn Chemistry

Q1.

How many moles are there in 40 g of H₂SO₄?
(Answer: 0.408 mole)

Q2.

Calculate the number of moles in 53 g of Na₂CO₃ and 36 g of water.
(Answer: 0.5 mole, 2 mole)

Q3.

Calculate the mass of one atom of carbon and one molecule of water.
(Answer: 1.99 × 10^-23 g, 2.99 × 10^-23 g)

Q4.

Calculate the mass of 5 moles of glucose and 3 moles of table salt.
(Answer: 900 g, 175.5 g)

Q5.

Calculate the number of moles in 8.4 g of NaHCO₃ and 1.7 g of ammonia.
(Answer: 0.1 mole, 0.1 mole)

OR

Calculate the number of moles in 26 g of oxalic acid H₂C₂O₄.2H₂O and 6 g of carbon.

Q6.

Calculate the number of moles in 40 g of Na.
(Answer: 1.739 mole)

Q7.

What is the mass of 4 moles of CO₂?
(Answer: 176 g)

Q8.

Calculate the number of atoms present in 9.2 g of Calcium (Ca).
(Answer: 1.384 × 10²³ atoms of Ca)

Q9.

Calculate the number of moles and number of molecules present in 8 g of C₆H₁₂O₆.
(Answer: 0.04 mole, 2.40 × 10²² molecules)

Q10.

Calculate the number of moles in 30 g of H₃PO₄.
(Answer: 0.306 mole)

Q11.

A silver (Ag) coin has a mass of 8.5 g. Calculate the number of moles of silver present in the coin.
(Answer: 0.07 mole of silver)

Q12.

Calculate the number of moles, number of molecules and number of atoms present in 10 g of H₂SO₄.
(Answer: 0.10 mole, 6.02 × 10²² molecules, 4.214 × 10²³ atoms)

Q13.

Calculate the molar mass of the following:

• Glucose
• Sucrose
• Sulphuric acid
• Ethene
• Ferric sulphate, Fe₂(SO₄)₃

Q14.

Calculate the formula mass (a.m.u.) of the following:

• Al₂O₃
• MgCl₂
• NaCl
• KNO₃
• Washing Soda (Na₂CO₃.10H₂O)

Q15.

Calculate the molecular mass (a.m.u.) of the following:

• C₂H₅OH (Ethanol)
• H₂O (Water)
• NH₃ (Ammonia)
• CO₂ (Carbon dioxide)
• CH₃COOH (Acetic acid)
• HNO₃ (Nitric acid)
• C₆H₆ (Benzene)

Q16.

Calculate the number of moles and number of molecules present in the following:

(a) 16 g of H₂CO₃
Answer: 0.258 mole, 1.55 × 10²³ molecules

(b) 20 g of C₆H₁₂O₆
Answer: 0.111 mole, 6.68 × 10²² molecules

Q17.

How many litres of carbon dioxide would be produced if 0.450 mole of carbon monoxide reacts with excess oxygen at STP?
(Answer: 10.08 L of CO₂)

Chemical Equation:
2CO(g) + O₂(g) → 2CO₂(g)