CBSE MCQs On Mole Concept Class 11 With Answers

Welcome to our comprehensive guide on CBSE MCQs on Mole Concept Class 11 with Answers. In this resource, we delve into the fundamental principles of Mole concept class 11 mcq with answers, providing a plethora of multiple-choice questions (MCQs) to solidify your understanding.

From mole concept questions class 11 PDF to mole concept class 11 NCERT solutions, this guide encompasses a wide array of topics, ensuring thorough preparation. Explore our mole concept class 11 MCQ PDF for a structured approach to mastering this essential concept. Let’s dive in!

Mole Concept Multiple Choice Questions And Answers Pdf

Mole concept class 11 mcq with answers

Mole Concept Questions Class 11 With Answer

Q. What does Avogadro’s number represent?

A) The number of atoms in 1 mole of a substance

B) The number of molecules in 1 mole of a substance

C) The number of grams in 1 mole of a substance

D) The number of particles in 1 mole of a substance

Answer: A) The number of atoms in 1 mole of a substance

Q. Which of the following represents the Avogadro constant?

A) 6.022 × 10²³

B) 6.022 × 10²³

C) 6.002 × 10²³

D) 6.002 × 10²³

Answer: A) 6.022 × 10²³

Q. What is the molar mass of water (H2O)?

A) 16 g/mol

B) 18 g/mol

C) 20 g/mol

D) 22 g/mol

Answer: B) 18 g/mol

Q. What is the mass of 1 mole of carbon atoms (C)?

A) 12 g

B) 14 g

C) 16 g

D) 18 g

Answer: A) 12 g

Also Read: Mole Concept – Definition & Examples

Q. How many moles of oxygen (O2) molecules are there in 44 g of oxygen gas?

A) 1 mole

B) 2 moles

C) 3 moles

D) 4 moles

Answer: B) 2 moles

Q. What is the formula to calculate the number of moles?

A) Moles = Mass × Avogadro’s number

B) Moles = Mass / Molar mass

C) Moles = Volume × Density

D) Moles = Volume / Molar volume

Answer: B) Moles = Mass / Molar mass

Q. Which of the following represents the correct unit for molar mass?

A) g/mol

B) kg/mol

C) mol/g

D) mol/L

Answer: A) g/mol

Also Check: Mole Concept and Molar Mass

Q. What is the molar mass of sulfuric acid (H2SO4)?

A) 64 g/mol

B) 82 g/mol

C) 98 g/mol

D) 104 g/mol

Answer: D) 98 g/mol

Q. How many atoms are there in 1 mole of oxygen gas (O2)?

A) 6.022 × 10^23 atoms

B) 2.011 × 10^23 atoms

C) 3.204 × 10^23 atoms

D) 1.204 × 10^23 atoms

Answer: A) 6.022 × 10²³ atoms

Q. What is the empirical formula of a compound with 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass?

A) CH2O

B) C2H6O2

C) C3H9O3

D) C4H10O4

Answer: B) C₂H₆O₂

Q. How many grams of CO2 are produced when 72 g of methane (CH4) is completely burned in oxygen?

A) 72 g

B) 88 g

C) 144 g

D) 176 g

Answer: B) 88 g

Q. Which of the following gases has the highest molar mass?

A) Hydrogen (H2)

B) Nitrogen (N2)

C) Oxygen (O2)

D) Carbon dioxide (CO2)

Answer: D) Carbon dioxide (CO2)

Q. What is the molecular formula of a compound with an empirical formula CH2O and a molar mass of 180 g/mol?

A) C2H4O2

B) C3H6O3

C) C4H8O4

D) C5H10O5

Answer: C) C4H8O4

Q. How many moles of aluminum atoms are there in 54 g of aluminum (Al)?

A) 1 mole

B) 2 moles

C) 3 moles

D) 4 moles

Answer: A) 1 mole

Q. What is the mass of 3 moles of sodium chloride (NaCl)?

A) 58.5 g

B) 87.0 g

C) 175.5 g

D) 262.5 g

Answer: C) 175.5 g

Q. What is the volume occupied by 1 mole of any gas at STP (Standard Temperature and Pressure)?

A) 22.4 L

B) 24.0 L

C) 25.6 L

D) 26.8 L

Answer: A) 22.4 L

More Resources for Class 11

• NCERT Solutions for Class 11 Chemistry
• NCERT Solutions for Class 11 Physics
• NCERT Solutions for Class 11 Biology
• NCERT Solutions for Class 11 Maths

Q. How many grams of hydrogen gas (H2) are needed to react completely with 32 g of oxygen gas (O2) to form water (H2O)?

A) 2 g

B) 4 g

C) 8 g

D) 16 g

Answer: B) 4 g

Q. What is the mass of 0.5 moles of calcium carbonate (CaCO3)?

A) 25 g

B) 50 g

C) 75 g

D) 100 g

Answer: B) 50 g

Q. Which of the following represents the correct formula for calculating the number of particles?

A) Particles = Moles × Avogadro’s number

B) Particles = Mass × Avogadro’s number

C) Particles = Volume × Avogadro’s number

D) Particles = Pressure × Avogadro’s number

Answer: A) Particles = Moles × Avogadro’s number

Q. What is the percentage composition of carbon in carbon dioxide (CO2)?

A) 12%

B) 25%

C) 50%

D) 75%

Answer: C) 50%